A mixture consisting entirely of Li2CO3 + BaCO3 weighs 1.000 g and requires 15.00 mL of 1.000 N HCl for neutralization. Find the percentage of BaCO3 and of combined Li in the sample.
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1. A mixture consisting entirely of Li2CO3 + BaCO3 weighs 1.000 g and requires 15.00 mL of 1.000 N HCl for neutralization. Find the percentage of BaCO3 and of combined Li in the sample.
2. A mixture of pure BaCO3 and pure Na2CO3 weighs 1.000 g and has the total neutralizing power of 15.37 meq of CaCO3. Calculate the percentage of combined CO2 in the mixture and the weight of Li2CO3 that has the same neutralizing power as 1.000 g of the above mixture.
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- A mixture of pure BaCO3 and pure Na2CO3 weighs 1.000 g and has the total neutralizing power of 15.37 meq of CaCO3. Calculate the percentage of combined CO2 in the mixture and the weight of Li2CO3 that has the same neutralizing power as 1.000 g of the above mixture.0.9563 g KHCO3 (M.r.(KHCO3) = 100.12 g/mol (mg/mmol)) have measured, and 50.0 cm3 stock solution have been prepared from it. 10.00 cm3 individual samples from it was titrated with HCl titrant in order to determine its concentration. The average HCl consumption was 19.18 cm3. The same HCl solution with were used to determine the concentration of NaOH titrant. The base consumption for 20.00 cm3 HCl was 21.35 cm3 NaOH. 1. concentration of HCl 2. concentration of NaOHA mixture of pure BaCO3 and pure Na2CO3 weighs 1.000 g and has the total neutralizing power of 15.37 meq of CaCO3. Calculate the percentage of combined CO2 in the mixture and the weight of Li2CO3 that has the same neutralizing power as 1.000 g of the above mixture. Note: include up to 4 decimal places Please explain each step
- What is the pH of the solution after mixing 0.188 g of Mg(OH)2 (MW=58.321 g/mol) with 18.1 mL of 0.0173 M HCl? The resulting solution was diluted to 100 mL. Round your calculated value for pH to two figures to the right of the decimal point.Use the following atomic masses (in g/mol): Mg = 24.31; H = 1; S = 32.06; O = 16; Na = 23; Cl = 35. 45; Ca = 40.08; C = 12.01; N = 14.01; Mg = 24.31 5.A sample of Chlorpheniramine Maleate (99.82%) weighing 0.502g was assayed by non-aqueous titrimetry and was found to be equivalent to 22.2mL of perchloric acid. Calculate for the normality of perchloric acid. Each mL of 0.1N perchloric acid is equivalent to 19.54mg of Chlorpheniramine Maleate.A 0.098 M K2Cr2O7 titrant was used for titration of 30 mL of aqueous Ethanol (C2H6O) solution and consumed 41.40 mL. (a) Calculate the mass of Ethanol and (b) determine degree proof of ethanol (density of pure ethanol= 0.789 g/mL).
- The protein content of wheat flour can be determined reasonably accurately by multiplying the percentage of nitrogen present by 5.7. A 2.06-g sample of flour was taken through a Kjeldahl procedure and the ammonia produced was distilled into a boric acid solution. If this solution required 34.70 mL of 0.174 N HCl for titration to the methyl red end point, what is the a) % Nitrogen and b) % protein in the flour? (Use 1:1 stoich ratio between N and HCl)A mixture of pure BaCO3 and pure Na2CO3 weighs 1.000 g and has the total neutralizing power of 15.37 meq of CaCO3. Calculate the percentage of combined CO2 in the mixture and the weight of Li2CO3 that has the same neutralizing power as 1.000 g of the above mixture. Instructions: Include up to 4 decimal places See sample photo for the format of solutionDetermine the required grams of a solid organic acid (KHP – 204.2 g/mol) that used as a primary standard to standardize and neutralize a base such as NaOH which is 1.005 mol/L. the volume you can assume
- Detailed calculations on how to prepare the solutions listed below Solution: 50 mL 1 M oxalic acid Oxalic acid Mw = 90.03 g mol-1 Oxalic acid purity = 98% Solution: 10 mL 3 M sulfuric acid Sulfuric acid Mw = 98.079 g mol-1 Sulfuric acid density = 1.84 g mL-1 Sulfuric acid purity = 98% Solution: 10 mL saturated potassium oxalate potassium oxalate (monohydrate used) Mw = 184.23 g mol-1 Solubility of potassium oxalate in water at 25°C = 360 mg mL-1 Solution :20 mL 3% hydrogen peroxide Hydrogen peroxide is commercially available as a 32% solution.Calculations for Acetate Buffer Solutions Molarity of acetic in acetate buffer (below is the data to answer the answer) Deionized water Acetate Buffer Ammonia Buffer pH of solution 6.62 4.59 9.49 Ph of solution after addition of 1 mL of 0.6 M NaOH 12.41 4.71 9.50 pH of solution after addition of 1 mL of 0.6 M HCl 1.38 3.87 9.24 Preparation of Buffer solutions Mass of sodium acetate in acetate buffer ~ 1.1981 Volume of 3.0 M acetic acid in acetate buffrer ~ 3.81 Mass of ammonium chloride ~ 1.2721 Volume of 5.0 M NH4OH ~ 6.00A mixture containing only KCl and NaBr is analyzed by the Mohr method. A 0.5072-g sample is dissolved in 50 mL of water and titrated to the Ag2CrO4 end point, requiring 36.85 mL of 0.1120 M AgNO3. A blank titration requires 0.71 mL of titrant to reach the same end point. Report the %w/w KCl and NaBr in the sample.KCl = 74.551 NaBr = 102.89