1a. At the endpoint in the titration of sodium hydroxide with sulfuric acid a. t
ID: 501088 • Letter: 1
Question
1a. At the endpoint in the titration of sodium hydroxide with sulfuric acid
a. the moles of H+ added to the solution are twice the moles of hydroxide added.
b. the moles of H+ added to the solution are the same the moles of hydroxide added.
c. the amount of water added to dilute the initial acid affects the amount of base required to reach the endpoint.
1b. At the endpoint of a titration between hydrochloric acid (HCl) and potassium hydroxide (KOH)
a. the moles of added base equal twice the moles of added acid.
b. the moles of added base equal the moles of added acid
1c. Calculate the concentration of a hydrobromic acid solution necessary to titrate a standard base of 1.243 x 10-1 M potassium hydroxide. The volume of base was 34.12 mL and acid was 85.01 mL
a. 2901 M HBr
b. 0.04989 M HBr
c. 0.3091 M HBr
1d. Calculate the number of moles of hydroxide anions per mL in a solution of 1.243 x 10-1 M potassium hydroxide standard.
a. 0.0001243 moles OH-
b. 1 moles OH-
c. 0.1243 moles OH-
1e. How many mL of 1.243 x 10-1 M cesium hydroxide are necessary to titrate 25.00 mL of 0.3400 M acid. The acid is monoprotic.
a. 58.13 ml
b. 25.00 ml
c. 68.38 ml
1f. The stoichiometry of a monoprotic acid titrated with a monohydroxy base is 1:1. What is the stoichiometry of a monoprotic acid titrated with a dihydroxy base?
a. 2:1
b. 1:1
Explanation / Answer
1a).
answer : a. the moles of H+ added to the solution are twice the moles of hydroxide added.
1b). At the endpoint of a titration between hydrochloric acid (HCl) and potassium hydroxide (KOH)
answer : b. the moles of added base equal the moles of added acid
1c.) answer : b. 0.04989 M HBr
M1 V1 = M2 V2
1.243 x 10^-1 x 34.12 = M2 x 85.01
M2 = 0.04989 M
1d) answer : c). 0.1243 moles OH-
moles of OH- = 1.243 x 10^-1
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