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12 Nov 2019

A 25.0 ml sample of 0.0750 M solution of Ba(OH)2 is titrated with 0.200 M HCl. How many milliliters of the HCl solution are required to reach the equivalence point of the titration?

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Irving Heathcote
Irving HeathcoteLv2
3 Jan 2019

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Related questions

. 12.75 grams of KOH are diluted to 125.0 ml with water. 10.0 ml of the resulting solution are removed and diluted to a final volume of 250.0 ml. What is the concentration of KOH in the final solution?

2. A 25.0 ml sample of 0.0750 M solution of Ba(OH)2 is titrated with 0.200 M HCl. How many milliliters of the HCl solution are required to reach the equivalence point of the titration?

3. For each of the weak acids listed below, a) write a balanced equilibrium equation showing the dissociation and b) write the equilibrium constant expression and c) give the Ka value (from your lecture note manual). HClO2 (aq) HC7H5O2 (aq) (also written as, C6H5COOH) HIO4 (aq)

4. A 150.0 ml sample of 0.250 M HCN is titrated with 50.0 ml of 0.200 M NaOH. What are the concentrations of HCN and CN in solution after the neutralization reaction occurs?

1. A 100 mL solution of 0.200 M HF is titrated with 0.100 M Ba(OH)2. What is the volume of Ba(OH)2 needed to reach equivalence point?

200 mL

50 mL

100 mL

300 mL

Cannot determine based on the provided information.

2. A 100 mL solution of 0.200 M NH3 is titrated with 0.100 M HCl. What is the volume of HCl needed to reach equivalence point?

200 mL

100 mL

50 mL

300 mL

Cannot determine based on the provided information.

3. A 100 mL solution of 0.200 M NH3 is titrated with 0.100 M HF. What is the volume of HF needed to reach equivalence point?

100 mL

50 mL

300 mL

Cannot determine based on the provided information.

4. A 100 mL solution of 0.200 M Sr(OH)2 is titrated with 0.100 M H3PO4. What is the volume of H3PO4 needed to reach equivalence point?

100 mL

200 mL

50 mL

300 mL

133 mL

5. A 100 mL solution of unknown concentration H2SO4 is titrated with 200 mL of 0.100 M Ba(OH)2 solution to reach equivalence point. What is the concentration of H2SO4 solution?

0.100 M

0.050 M

0.020 M

0.200 M

Cannot determine based on the provided information.

6. A 100 mL solution of unknown concentration H3PO4 is titrated with 200 mL of 0.100 M Sr(OH)2 solution to reach equivalence point. What is the concentration of H3PO4 solution?

0.100 M

0.133 M

0.200 M

0.050 M

0.300 M

A 100 mL solution of 0.200 M HF(Ka=6.6*10-4) is titrated with 0.100 M Ba(OH)2. It takes 100 mL of Ba(OH)2 to reach the equivalence point. What is the pH at half-equivalence point?

7

3.5

3.18

10.5

10.82

8. Based on your answer in #7, what is the concentration of H3O+ at half-equivalence point?

6.6 × 10-4 M

6.61 × 10-4 M

10-7 M

3.2 × 10-4 M

3.16 × 10-4 M

9. A 100 mL solution of 0.200 M unknown weak acid is titrated with 0.100 M NaOH. The pH at half-equivalence point is 5.52. What is the Ka value for the unknown weak acid?

3.02 × 10-6

3.31 × 105

3.0 × 10-6

3.3 × 105

Cannot determine based on the provided information.

10. Based on your answer in #9, what is the concentration of H3O+ at half-equivalence point?

3.0 × 10-6

3.02 × 10-6

3.31 × 105

3.3 × 105

Cannot determine based on the provided information

A 50.0-mL sample of a 0.100 M solution of NaCN is titrated by 0.200 M HCl.

Kb for CN− is 2.0×10−5. Calculate the pH of the solution:

  1. Prior to the start of the titration
  2. After the addition of 15.0 mL of 0.200 M HCl
  3. At the equivalence point
  4. After the addition of 30.0 mL of 0.200 M HCl

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