An important limitation when using an indicator is that we must be able to see the indicators change in color at the end point. endstream endobj 244 0 obj <>/Metadata 80 0 R/Pages 79 0 R/StructTreeRoot 82 0 R/Type/Catalog/ViewerPreferences<>>> endobj 245 0 obj <>/ExtGState<>/Font<>/ProcSet[/PDF/Text]>>/Rotate 0/StructParents 0/TrimBox[0.0 0.0 595.276 841.89]/Type/Page>> endobj 246 0 obj <> endobj 247 0 obj <>stream |" " " " " " " # # # # # >$ {l{]K=/=h0Z CJ OJ QJ ^J aJ h)v CJ OJ QJ ^J aJ #hk hk 5CJ OJ QJ ^J aJ h 5CJ OJ QJ ^J aJ h)v 5CJ OJ QJ ^J aJ hL 5CJ OJ QJ ^J aJ hk CJ OJ QJ ^J aJ hH CJ OJ QJ ^J aJ hlx% CJ OJ QJ ^J aJ hlx% hlx% CJ OJ QJ ^J aJ hlx% hH CJ OJ QJ ^J aJ (h- hH CJ OJ QJ ^J aJ mHsH (hk hk CJ OJ QJ ^J aJ mHsH>$ ?$ % % P OQ fQ mQ nQ R yS zS T T T U U U U U U U U U U !U 8U 9U :U ;U =U ?U @U xj j h7 UmH nH u h? After the equivalence point the absorbance remains essentially unchanged. ^208u4-&2`jU" JF`"Py~}L5@X2.cXb43{b,cbk X$ ! The solution was diluted to 500 ml, and 50 ml was pipetted and heated to boiling with 2.5 ml of 5% ammonium oxalate solution. For example, after adding 5.0 mL of EDTA, the total concentration of Cd2+ is, \[\begin{align} 2.1 The magnesium EDTA exchanges magnesium on an equivalent basis for any calcium and/or other cations to form a more stable EDTA chelate than magnesium. It is a method used in quantitative chemical analysis. Add a pinch of Eriochrome BlackT ground with sodium chloride (100mg of indicator plus 20g of analytical grade NaCl). Because not all the unreacted Cd2+ is freesome is complexed with NH3we must account for the presence of NH3. 0000002315 00000 n Indicator. 0000000961 00000 n Estimation of Copper as Copper (1) thiocyanate Gravimetry, Estimation of Magnesium ions in water using EDTA, Organic conversion convert 1-propanol to 2-propanol. \end{align}\], \[\begin{align} See the final side comment in the previous section for an explanation of why we are ignoring the effect of NH3 on the concentration of Cd2+. From Table 9.10 and Table 9.11 we find that Y4 is 0.35 at a pH of 10, and that Cd2+ is 0.0881 when the concentration of NH3 is 0.0100 M. Using these values, the conditional formation constant is, \[K_\textrm f''=K_\textrm f \times \alpha_\mathrm{Y^{4-}}\times\alpha_\mathrm{Cd^{2+}}=(2.9\times10^{16})(0.37)(0.0881)=9.5\times10^{14}\], Because Kf is so large, we can treat the titration reaction, \[\textrm{Cd}^{2+}(aq)+\textrm Y^{4-}(aq)\rightarrow \textrm{CdY}^{2-}(aq)\]. More than 95% of calcium in our body can be found in bones and teeth. h% CJ OJ QJ ^J aJ h`. Architektw 1405-270 MarkiPoland, free trial version of the stoichiometry calculator. 0000028404 00000 n Hardness EDTA as mg/L CaCO3 = (A*B*1000)/ (ml of Sample) Where: A = ml EDTA Solution Used. Although EDTA is the usual titrant when the titrand is a metal ion, it cannot be used to titrate anions. Calculate titration curves for the titration of 50.0 mL of 5.00103 M Cd2+ with 0.0100 M EDTA (a) at a pH of 10 and (b) at a pH of 7. Calcium and Magnesium Determinations by EDTA Titrations A scout titration is performed to determine the approximate calcium content. Determination of Total hardness Repeat the above titration method for sample hard water instead of standard hard water. leaving 4.58104 mol of EDTA to react with Cr. (Use the symbol Na 2 H 2 Y for Na 2 EDTA.) Estimation of magnesium ions using edta. PDF Experiment 7 - University of Idaho 0000021941 00000 n Add 10 mL of ammonia buffer, 50 mL of distilled water and 1 mL of Eriochrome Black T indicator By direct titration, 5 ml. Answer Mol arity EDTA (m ol / L) = Volume Zinc ( L) Mol rity m l / 1 mol EDTA 1 mol Zinc 1 . Complexometric determination of magnesium oxide in flyash - PubMed When the reaction is complete all the magnesium ions would have been complexed with EDTA and the free indicator would impart a blue color to the solution. 0000009473 00000 n where VEDTA and VCu are, respectively, the volumes of EDTA and Cu. For each of the three titrations, therefore, we can easily equate the moles of EDTA to the moles of metal ions that are titrated. This displacement is stoichiometric, so the total concentration of hardness cations remains unchanged. Titration . This can be done by raising the pH to 12, which precipitates the magnesium as its hydroxide: Mg2+ + 2OH- Mg(OH) 2 EDTA. Determination of Total Hardness of Water The objective of Table B of the experiment is to determine the total hardness of the given water samples: well water, tap water, and seawater. trailer PDF Determination of water hardness from common water sources using flame of standard calcium solution are assumed equivalent to 7.43 ml. 0000001334 00000 n Other absorbing species present within the sample matrix may also interfere. Why is the sample buffered to a pH of 10? You can review the results of that calculation in Table 9.13 and Figure 9.28. To maintain a constant pH during a complexation titration we usually add a buffering agent. PDF Method 130.1 Hardness, Total (mg/L as CaCO3) (Colorimetric, Automated PDF CEL212 Environmental Engineering Second Semester 2012-13 Laboratory Most indicators for complexation titrations are organic dyesknown as metallochromic indicatorsthat form stable complexes with metal ions. Titration is a method to determine the unknown concentration of a specific substance (analyte) dissolved in a sample of known concentration. As shown in the following example, we can easily extended this calculation to complexation reactions using other titrants. This means that the same concentration of eluent is always pumped through the column. Although most divalent and trivalent metal ions contribute to hardness, the most important are Ca2+ and Mg2+. Even if a suitable indicator does not exist, it is often possible to complete an EDTA titration by introducing a small amount of a secondary metalEDTA complex, if the secondary metal ion forms a stronger complex with the indicator and a weaker complex with EDTA than the analyte. Report the molar concentration of EDTA in the titrant. Reactions taking place Chloride is determined by titrating with Hg(NO3)2, forming HgCl2(aq). About Press Copyright Contact us Creators Advertise Developers Terms Privacy Policy & Safety How YouTube works Test new features NFL Sunday Ticket Press Copyright . CJ OJ QJ ^J aJ hLS CJ OJ QJ ^J aJ h, h% CJ OJ QJ ^J aJ h- CJ OJ QJ ^J aJ t v 0 6 F H J L N ` b B C k l m n o r #hH hH >*CJ OJ QJ ^J aJ hH CJ OJ QJ ^J aJ hk hH CJ OJ QJ ^J aJ h% CJ OJ QJ ^J aJ hLS h% CJ OJ QJ ^J aJ hLS CJ OJ QJ ^J aJ h, h% CJ OJ QJ ^J aJ hp CJ OJ QJ ^J aJ h, h% CJ OJ QJ ^J aJ $ 1 4  |n||||]]||n| h, h% CJ OJ QJ ^J aJ hLS CJ OJ QJ ^J aJ hp CJ OJ QJ ^J aJ h, h% CJ OJ QJ ^J aJ hk hk CJ OJ QJ ^J aJ h% CJ OJ QJ ^J aJ #h hH CJ H*OJ QJ ^J aJ hH CJ OJ QJ ^J aJ #hH hH >*CJ OJ QJ ^J aJ &h hH >*CJ H*OJ QJ ^J aJ !o | } In the method described here, the titrant is a mixture of EDTA and two indicators. Titration is one of the common method used in laboratories which determines the unknown concentration of an analyte that has been identified. Problem 9.42 from the end of chapter problems asks you to verify the values in Table 9.10 by deriving an equation for Y4-. A more recent method is the titration of magnesium solution with ethylene-diamine tetra-acetate(Carr and Frank, 1956). of which 1.524103 mol are used to titrate Ni. If the metalindicator complex is too strong, the change in color occurs after the equivalence point. (Show main steps in your calculation). PDF Experiment2 Analysis*of*magnesium* The specific form of EDTA in reaction 9.9 is the predominate species only at pH levels greater than 10.17. The correction factor is: f = [ (7.43 1.5)/51/2.29 = 0.9734 The milliliters of EDTA employed for the calcium and the calcium plus mag- nesium titration are nmltiplied by f to correct for precipitate volume. EDTA Titration: Calcium in Calcium Supplements Student Handout Purpose To determine the amount of calcium in a calcium supplement tablet by EDTA titration. 2ml of serum contains Z mg of calcium. See Chapter 11 for more details about ion selective electrodes. Because EDTA forms a stronger complex with Cd2+ it will displace NH3, but the stability of the Cd2+EDTA complex decreases. Determination of Total Hardness by Titration with Standardized EDTA Determine the total hardness (Ca2+ and Mg2+) by using a volumetric pipet to pipet 25 mL of the unknown solution into a 250 mL Erlenmeyer flask. Why is a small amount of the Mg2+EDTA complex added to the buffer? Read mass of magnesium in the titrated sample in the output frame. Figure 9.34 Titration curves illustrating how we can use the titrands pH to control EDTAs selectivity. Repeat the titration twice. Figure 9.33 shows the titration curve for a 50-mL solution of 103 M Mg2+ with 102 M EDTA at pHs of 9, 10, and 11. \[\alpha_{\textrm Y^{4-}} \dfrac{[\textrm Y^{4-}]}{C_\textrm{EDTA}}\tag{9.11}\]. See Figure 9.11 for an example. After adding calmagite as an indicator, the solution was titrated with the EDTA, requiring 42.63 mL to reach the end point. Complexometric determination of calcium - Titration and titrimetric methods %%EOF 0000001156 00000 n ! The stoichiometry between EDTA and each metal ion is 1:1. Why does the procedure specify that the titration take no longer than 5 minutes? General chemistry 1 analytic report - Experiment 9 DETERMINATION OF (b) Titration of a 50.0 mL mixture of 0.010 M Ca2+ and 0.010 M Ni2+ at a pH of 3 and a pH of 9 using 0.010 M EDTA. Dilutes with 100 ml of water and titrate the liberated iodine with 0.1M sodium thiosulphate using 0.5ml of starch solution, added towards the end of the titration, as an indicator. ^.FF OUJc}}J4 z JT'e!u3&. Compare your results with Figure 9.28 and comment on the effect of pH and of NH3 on the titration of Cd2+ with EDTA. A indirect complexation titration with EDTA can be used to determine the concentration of sulfate, SO42, in a sample. The experimental approach is essentially identical to that described earlier for an acidbase titration, to which you may refer. C_\textrm{Cd}&=\dfrac{\textrm{initial moles Cd}^{2+} - \textrm{moles EDTA added}}{\textrm{total volume}}=\dfrac{M_\textrm{Cd}V_\textrm{Cd}-M_\textrm{EDTA}V_\textrm{EDTA}}{V_\textrm{Cd}+V_\textrm{EDTA}}\\ (mg) =Volume. \[\textrm{MIn}^{n-}+\textrm Y^{4-}\rightarrow\textrm{MY}^{2-}+\textrm{In}^{m-}\]. OJ QJ UmH nH u h CJ OJ QJ ^J aJ h, h% CJ OJ QJ ^J aJ hs CJ OJ QJ ^J aJ R T V Z v x | qcU? EDTA Titration Calculations The hardness of water is due in part to the presence of Ca2+ ions in water. Complexometric titration is used for the estimation of the amount of total hardness in water. Practical analytical applications of complexation titrimetry were slow to develop because many metals and ligands form a series of metalligand complexes. It is vital for the development of bones and teeth. xref Obtain a small volume of your unknown and make a 10x dilution of the unknown. (a) Titration of 50.0 mL of 0.010 M Ca2+ at a pH of 3 and a pH of 9 using 0.010 M EDTA. 3. and pCd is 9.77 at the equivalence point. A buffer solution is prepared for maintaining the pH of about 10. Repeat the titrations to obtain concordant values. 0000000016 00000 n HWM6W- ~jgvuR(J0$FC*$8c HJ9b\I_~wfLJlduPl 0000007769 00000 n Complexation Titration: Determination of Total Hardness of Water A 0.4482-g sample of impure NaCN is titrated with 0.1018 M AgNO3, requiring 39.68 mL to reach the end point. EDTA Titration for Determination of calcium and magnesium The obtained average molarity of EDTA (0.010070.00010 M) is used in Table 2 to determine the hardness of water. Although many quantitative applications of complexation titrimetry have been replaced by other analytical methods, a few important applications continue to be relevant. PDF Experiment 5 EDTA Titration: Calcium in Calcium Supplements Thus one simply needs to determine the area under the curve of the unknown and use the calibration curve to find the unknown concentration. This is often a problem when analyzing clinical samples, such as blood, or environmental samples, such as natural waters. Figure 9.35 Spectrophotometric titration curve for the complexation titration of a mixture of two analytes. Cyanide is determined at concentrations greater than 1 mg/L by making the sample alkaline with NaOH and titrating with a standard solution of AgNO3, forming the soluble Ag(CN)2 complex. Contrast this with Y4-, which depends on pH. Calcium. Solutions of Ag+ and Hg2+ are prepared using AgNO3 and Hg(NO3)2, both of which are secondary standards. The evaluation of hardness was described earlier in Representative Method 9.2. EDTA Titration You would like to perform a titration of 50.00 mL of a 1.00 x 10-4 M Zn2+ solution with a 1.00 x 10-4 M EDTA solution. Another common method is the determination by . Magnesium. 4! Add 10 mL of pH 10 NH4/NH4OH buffer and 10 mg of ascorbic acid just before titrating. Complexometric Determination of Magnesium using EDTA EDTA Procedure Ethylenediaminetetraacetic Acid Procedure Preparing a Standard EDTA Solution Reactions 1.Weighing by difference 0.9g of EDTA 2.Quantitatively transfer it to a 250 mL volumetric flask 3.Add a 2-3mL of amonia buffer (pH 10) ! All Answers (10) 1) Be sure the pH is less than 10, preferably about 9.5-9.7. nn_M> hLS 5CJ OJ QJ ^J aJ #h, hLS 5CJ OJ QJ ^J aJ hLS 5CJ OJ QJ ^J aJ &h, h% 5CJ H*OJ QJ ^J aJ #h, h% 5CJ OJ QJ ^J aJ #hk hk 5CJ OJ QJ ^J aJ h, h% CJ OJ QJ ^J aJ h h (j h? The procedure de-scribed affords a means of rapid analysis. How do you calculate the hardness of water in the unit of ppm #MgCO_3#? startxref The resulting metalligand complex, in which EDTA forms a cage-like structure around the metal ion (Figure 9.26b), is very stable. which is the end point. For removal of calcium, three precipitation procedures were compared. Select a volume of sample requiring less than 15 mL of titrant to keep the analysis time under 5 minutes and, if necessary, dilute the sample to 50 mL with distilled water. The EDTA was standardized by the titration method as well. The sample is acidified to a pH of 2.33.8 and diphenylcarbazone, which forms a colored complex with excess Hg2+, serves as the indicator. If preparation of such sample is difficult, we can use different EDTA concentration. 0000001920 00000 n \[K_\textrm f''=\dfrac{[\mathrm{CdY^{2-}}]}{C_\textrm{Cd}C_\textrm{EDTA}}=\dfrac{3.33\times10^{-3}-x}{(x)(x)}= 9.5\times10^{14}\], \[x=C_\textrm{Cd}=1.9\times10^{-9}\textrm{ M}\]. To evaluate the titration curve, therefore, we first need to calculate the conditional formation constant for CdY2. The solution is warmed to 40 degrees C and titrated against EDTA taken in the burette. Click here to review your answer to this exercise. PDF Determination of Calcium, Magnesium, and Sodium by Atomic Spectrophotometry The reaction between Cl and Hg2+ produces a metalligand complex of HgCl2(aq). Water Hardness (EDTA) Titration Calculations Example - YouTube If MInn and Inm have different colors, then the change in color signals the end point. A comparison of our sketch to the exact titration curve (Figure 9.29f) shows that they are in close agreement. Detection is done using a conductivity detector. If desired, calcium could then be estimated by subtracting the magnesium titration (d) from the titration for calcium plus magnesium (a). Adjust the samples pH by adding 12 mL of a pH 10 buffer containing a small amount of Mg2+EDTA. to the EDTA titration method for the determination of total hardness, based on your past experience with the ETDA method (e.g., in CH 321.) A 0.1557-g sample is dissolved in water, any sulfate present is precipitated as BaSO4 by adding Ba(NO3)2. %PDF-1.4 % Complexation titrimetry continues to be listed as a standard method for the determination of hardness, Ca2+, CN, and Cl in waters and wastewaters. Determining Calcium Ion Concentration in Water Chemistry Tutorial The end point occurs when essentially all of the cation has reacted. teacher harriet voice shawne jackson; least stressful physician assistant specialties; grandma's marathon elevation gain; describe key elements of partnership working with external organisations; When the titration is complete, we adjust the titrands pH to 9 and titrate the Ca2+ with EDTA. Hardness is mainly the combined constituent of both magnesium and calcium. Method C, the EDTA titration method, measures the calcium and magnesium ions and may be applied with appro-priate modication to any kind of water. EDTA solution. We will use this approach when learning how to sketch a complexometric titration curve. Magnesium levels in drinking water in the US. Our goal is to sketch the titration curve quickly, using as few calculations as possible. Determination of Mg by Titration with EDTA INTRODUCTION The titration is done with 0.1 mol/l AgNO3 solution to an equivalence point. Eriochrome Black-T(EBT) is the metal ion indicator used in the determination of hardness by complexometric titration with EDTA. H|W$WL-_ |`J+l$gFI&m}}oaQfl%/|}8vP)DV|{*{H [1)3udN{L8IC 6V ;2q!ZqRSs9& yqQi.l{TtnMIrW:r9u$ +G>I"vVu/|;G k-`Jl_Yv]:Ip,Ab*}xqd e9:3x{HT8| KR[@@ZKRS1llq=AE![3 !pb 0000011407 00000 n \[\begin{align} 0000008621 00000 n lab report 6 determination of water hardness Step 4: Calculate pM at the equivalence point using the conditional formation constant. Erlenmeyer flask. PDF Determination of Mg by Titration with EDTA - Truman State University The red points correspond to the data in Table 9.13. In an acid-base titration, the titrant is a strong base or a strong acid, and the analyte is an acid or a base, respectively. PDF EDTA Titrations 2: Analysis of Calcium in a Supplement Tablet; Analysis [Simultaneous determination of calcium and magnesium by - PubMed If the sample does not contain any Mg2+ as a source of hardness, then the titrations end point is poorly defined, leading to inaccurate and imprecise results. The resulting analysis can be visualized on a chromatogram of conductivity versus time. PDF Calcium Analysis by EDTA Titration - Community College of Rhode Island As we add EDTA it reacts first with free metal ions, and then displaces the indicator from MInn. A time limitation suggests that there is a kinetically controlled interference, possibly arising from a competing chemical reaction. How do you calculate EDTA titration? 0000022320 00000 n 5CJ OJ QJ ^J aJ h`. For example, calmagite gives poor end points when titrating Ca2+ with EDTA. Thus, when the titration reaches 110% of the equivalence point volume, pCd is logKf 1. PDF EDTA Titration Calculations - Community College of Rhode Island The sample was acidified and titrated to the diphenylcarbazone end point, requiring 6.18 mL of the titrant. After transferring a 50.00-mL portion of this solution to a 250-mL Erlenmeyer flask, the pH was adjusted by adding 5 mL of a pH 10 NH3NH4Cl buffer containing a small amount of Mg2+EDTA. 2 23. The titration uses, \[\mathrm{\dfrac{0.05831\;mol\;EDTA}{L}\times 0.02614\;L\;EDTA=1.524\times10^{-3}\;mol\;EDTA}\]. mole( of( EDTA4-perliter,and&VEDTA( is( the( volume( of EDTA 4- (aq)inunitsofliter neededtoreachtheendpoint.If( you followed instructions, V Mg =0.025Land( C EDTA =( The titration can be carried out with samples with chloride contents of a few ppm - 100%, but the amount of sample has to be adjusted. The buffer is at its lower limit of pCd = logKf 1 when, \[\dfrac{C_\textrm{EDTA}}{[\mathrm{CdY^{2-}}]}=\dfrac{\textrm{moles EDTA added} - \textrm{initial moles }\mathrm{Cd^{2+}}}{\textrm{initial moles }\mathrm{Cd^{2+}}}=\dfrac{1}{10}\], Making appropriate substitutions and solving, we find that, \[\dfrac{M_\textrm{EDTA}V_\textrm{EDTA}-M_\textrm{Cd}V_\textrm{Cd}}{M_\textrm{Cd}V_\textrm{Cd}}=\dfrac{1}{10}\], \[M_\textrm{EDTA}V_\textrm{EDTA}-M_\textrm{Cd}V_\textrm{Cd}=0.1 \times M_\textrm{Cd}V_\textrm{Cd}\], \[V_\textrm{EDTA}=\dfrac{1.1 \times M_\textrm{Cd}V_\textrm{Cd}}{M_\textrm{EDTA}}=1.1\times V_\textrm{eq}\]. To prevent an interference the pH is adjusted to 1213, precipitating Mg2+ as Mg(OH)2. The most likely problem is spotting the end point, which is not always sharp. Add 4 drops of Eriochrome Black T to the solution. The indicator, Inm, is added to the titrands solution where it forms a stable complex with the metal ion, MInn. At a pH of 9 an early end point is possible, leading to a negative determinate error. We begin by calculating the titrations equivalence point volume, which, as we determined earlier, is 25.0 mL. 3: Hardness (in mg/L as CaCO 3 . Sample amount for titration with 0.1 mol/l AgNO 3 Chloride content [%] Sample [g] < 0.1 > 10 a mineral analysis is performed, hardness by calculation can be reported. Determination of Calcium and Magnesium in Milk by E.D.T.A. Titration 0000023545 00000 n If at least one species in a complexation titration absorbs electromagnetic radiation, we can identify the end point by monitoring the titrands absorbance at a carefully selected wavelength. 2. Calculate the number of grams of pure calcium carbonate required to prepare a 100.0 mL standard calcium solution that would require ~35 mL of 0.01 M EDTA for titration of a 10.00 mL aliquot: g CaCO 3 = M EDTA x 0.035L x 1 mol CaCO 3/1 mol EDTA x MM CaCO 3 x 100.0mL/10.00mL 3. zhVGV9 hH CJ OJ QJ ^J aJ h 5CJ OJ QJ ^J aJ #h hH 5CJ OJ QJ ^J aJ #hk h(5 5CJ OJ QJ ^J aJ h(5 CJ OJ QJ ^J aJ $h(5 h(5 5B* This is how you can perform an estimation of magnesium using edta. Sketch titration curves for the titration of 50.0 mL of 5.00103 M Cd2+ with 0.0100 M EDTA (a) at a pH of 10 and (b) at a pH of 7. in triplicates using the method of EDTA titration. PDF Determination!of!calcium!by!Standardized!EDTASolution! Introduction Figure 9.28 Titration curve for the titration of 50.0 mL of 5.00103 M Cd2+ with 0.0100 M EDTA at a pH of 10 and in the presence of 0.0100 M NH3. A titration of Ca2+ at a pH of 9 gives a distinct break in the titration curve because the conditional formation constant for CaY2 of 2.6 109 is large enough to ensure that the reaction of Ca2+ and EDTA goes to completion. [\mathrm{CdY^{2-}}]&=\dfrac{\textrm{initial moles Cd}^{2+}}{\textrm{total volume}}=\dfrac{M_\textrm{Cd}V_\textrm{Cd}}{V_\textrm{Cd}+V_\textrm{EDTA}}\\ Ethylenediaminetetraacetate (EDTA) complexes with numerous mineral ions, including calcium and magnesium. 5. You will work in partners as determined by which unknown was chosen. In addition magnesium forms a complex with the dye Eriochrome Black T. The determination of the Calcium and Magnesium next together in water is done by titration with the sodium salt of ethylenediaminetetraethanoic acid (EDTA) at pH 8 9, the de- tection is carried out with a Ca electrode. Add 1 or 2 drops of the indicator solution. Titration 2: moles Ni + moles Fe = moles EDTA, Titration 3: moles Ni + moles Fe + moles Cr + moles Cu = moles EDTA, We can use the first titration to determine the moles of Ni in our 50.00-mL portion of the dissolved alloy. A 0.4071-g sample of CaCO3 was transferred to a 500-mL volumetric flask, dissolved using a minimum of 6 M HCl, and diluted to volume.
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