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What is the acetate ion concentration, [C2H3O21-] of a 100mL of calcium acetate solution, Ca(C2H3O2)2, with 25.0g dissolved Ca(C2H3O2)2?
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- 25 g of the dilute mixture of H2SO4 and HNO3 is completed to 500 mL with water. When BaCl2 is added to 10 mL of this solution, the precipitate obtained is 362 mg. Another 20 mL portion taken from the solution is neutralized with 39.2 mL of 0.2 M NaOH solution in the presence of phenolphthalein. Calculate the percentage of HNO3 in the starting mixture.A 1.43 x 10-4 L solution of 45.7 mg/mL protein was analyzed using the Kjeldahl procedure. After digestion of the protein, the liberated NH3 was collected in 9.80 mL of 0235 M HCl. The unreacted acid required 10.75 mL of a standard solution of 0.0149 M NaOH for complete titration. Calculate the weight percent of nitrogen in the protein. (Molar mass N = 14.00674 g/mol)4a) Write an equation for the neutralization reaction of sodium acetate in solution upon addition of HCl.
- A 2.00 mL sample of serum is analyzed for protein by the modified Kjeldahl method. The sample is digested and the resulting ammonia is distilled into a boric acid solution, consuming 15.0 mL of standard HCl to titrate the ammonium borate. HCl is standardized by treating 0.330 g of pure (NH₄)₂SO₄ in the same way. If 33.3 mL of acid is consumed in the standardization titration, what is the serum protein concentration in g% (wt/vol)?Assume that a sample of hard water contains 50. mg/L of Mg2+ and 150 mg/L of Ca2+, with HCO3 as the accompanying anion. What mass of CaO should be added to 1.0 L of this aqueous solution to precipitate all the Mg2+ and Ca2+ as CaCO3 and MgCO3? What is the total mass of the two solids formed?A solution contains a mixture of Na2CO3 and NaHCO3. Titration of a 30.0 mL portion of the solution to a phenolphthalein end point requires 12.16 mL of 0.306 M HCl. Another 30.0 mL portion of the solution requires 42.76 mL of the 0.306 M HCl when titrated to a bromocresol green end point. Calculate the molarity of the NaHCO3 in the original solution. Please keep your answer in normal number to three decimal places (x.xxx).
- Titration of a 0.824 g of 99.99% KHP (204.23 g/mol) with phenolphthalein required 18.3 mL of NaOH (40.00 g/mol) solution to reach the end point. The same titrant was used to analyze an impure acetic acid (CH3COOH, 60.06 g/mol) solution. A 10.0 mL aliquot of the sample required 12.9 mL of the titrant. What substance served as the primary standard?Which served as the indicator in the titration?What is the color at the end point?What is the concentration of the titrant?What is the molar concentration of the acetic acid solution?Ca3(PO4) ksp =2.07x10^-33 PbCl2 ksp= 1.70x10^-5 CaCl2 ksp= 1.63x10^3An impure sample of oxalis acid was oxidized by potassium permanganate. A 0.261g sample of oxalis acid was dissolved and the solution was diluted to 100ml. A 25.0 ml portion of the oxalis acid solution was titrated with 26.2ml of 0.0107M potassium permanganate. How many moles of oxalis acid were titrated and what is the percent purity of the oxalis acid sample?
- 2NaHCO3 \rightarrow→ Na2CO3 + CO2 + H2O Which type of chemical reaction does this chemical equation represent?Suppose that the solubility of calcium iodate are 2.5 g/L at 20oC and 5.5 g/L at 60oC. What are the solubility in mol/L at 20oC and at 60oC? How many milliliters (mL) of 0.045 M Na2S2O3 will be required to titrate a 10.0-mL sample of saturated Ca(IO3)2 solution collected at 20oC and 60oC, respectively?What is the equilibrium constant for the following reaction that occurs when disodium citrate(Na2HC6H5O7) dissolves in water at 25ºC? The acid dissociation constants for citric acid, H3C6H5O7 , are:Ka1 = 7.4 × 10–4 , Ka2 =1.7 × 10–5 , and Ka3 = 4.0 × 10–7 . HC6H5O72– (aq) + H2O(l) ⇌ H2C6H5O7– (aq) + OH– (aq)
