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If a water has a carbonate alkalinity of 120.00 mg/L as the ion and a pH of 10.30,
what is the bicarbonate alkalinity in mg/L as the ion
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- The titration of a 20.0mL sample of an H2SO4 solution of unkown concentration requires 22.87mL of a 0.518 M KOH solution to reach the equivalent point. What is the concentration of the unknown H2SO4 solution ?If 35.0 mL of a 0.100 N acid solution is needed to reach the end point in titration of 21.5 mL of a base solution, what is the normality of the base solution?A solution contains NaHCO3 (84.01 g/mol), Na2CO3 (105.99 g/mol), and NaOH (40.00 g/mol), either alone or in permissible combination. Titration of a 25.0-mL portion to a phenolphthalein end point requires 29.75 mL of 0.1205 M HCl. A second 25.0-mL aliquot requires 36.56 mL of the HCl when titrated to a bromocresol green end point. What is the general composition of the solution? Calculate the no. of mg of each solute per mL of solution.
- A water sample has exact alkalinity of 220 mg/L CaCO3. The sample contains150.0 mg/L HCO3 at a pH of 7.1 (Temperature = 25 oC).(a) Calculate the carbonate alkalinity in mg/L as CO3.2. To standardize a solution of NaOH, a student measured 0.326 g of potassium hydrogen phthalate (KHC8H404 or KHP) and dissolved it in 50.0 mL of water. To the solution, two drops of phenolphthalein indicator was added. To reach the equivalence point as indicated by endpoint of the titration where the solution retained a pale pink color, a volume of 15.3 mL was required. What is the molarity of the NaH solution? (KHP is a monoprotic acid that furnishes one H* ion; at the equivalence point, mols OH (base) = mols H* (acid))In standardizing a solution of NaOH against 1.431g of KHC8H4O4, the analyst uses 35.50 mL of the alkali and has to run back with 5.12 mL of acid ( 1mL ≎0.0031g Na2O) What is the normality of NaOH?
- Consider a buffer solution containing an acid with a pKa of 2.3 and an acid concentration that is one fourth the concentration of the conjugate base. What is the pH of the solution?A water sample from a river has a pH of 7. What species make up the carbonate system of this sample? And which ones contribute to the total alkalinity of this same sample?Titration of a 18.0 mL solution of KOH requires 11.0 mL of 0.0270 M H2SO4 solution. What is the molarity of the KOH solution?
- What is the caustic alkalinity of a solution with a carbonate concentration of 20 mg/L and a pH of 8.1 if it requires 20 mL of 0.10 M HCl to titrate this same sample from a pH of 7 down to a pH of 4.5?A student is conducting molecular weight determination of an unknown diprotic acid. He first prepared a 250 mL NaOH (39.997 g/mol) titrant solution, which he then standardized with 0.5830 g of KHP (204.22g/mol) which consumed 24.02 mL of the titrant. After standardization, he weighed 0.2108 g of unknown diprotic acid and the titration reached the endpoint at a volume of 21.58 mL. (a) What is the standardized concentration of the titrant? Choices: 0.1000 M 0.1189 M 0.1286 M 0.1419 M (b) What is the molar mass of the diprotic acid? Choices: 82.19 g/mol 137.68 g/mol 164.38 g/mol 195.37 g/molA student is conducting molecular weight determination of an unknown diprotic acid. He first prepared a 250 mL NaOH (39.997 g/mol) titrant solution, which he then standardized with 0.5830 g of KHP (204.22g/mol) which consumed 24.02 mL of the titrant. After standardization, he weighed 0.2108 g of unknown diprotic acid and the titration reached the endpoint at a volume of 21.58 mL. (a) What is the standardized concentration of the titrant? (b) What is the molar mass of the diprotic acid?