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2. A 16.0 mL aliquot of a 0.220 M solution of H2SO4 is titrated with a 0.211 M NaOH solution. What volume (mL) of base will it take to reach the equivalence point?

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Related questions

A volume of 90.0 mL of a 0.820 M HNO3 solution is titrated with 0.220 M KOH. Calculate the volume of KOH required to reach the equivalence point.

Express your answer to three significant figures and include the appropriate units.

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. A student obtains a vinegar solution having an acetic acidconcentration of 0.8512 M. What volume of 0.1036 M NaOH will berequired to reach the equivalence point when 25.00 mL of thevinegar solution is titrated?

b. A student dilutes the vinegar solution in part a above bypipetting 10 mL of the solution into a 100 mL volumetric flask anddiluting to a total volume of 100 mL. What volume of 0.1036 M NaOHwill be required to reach the equivalence point when 100 mL of thediluted vinegar solution is titrated?

c. What volume of 0.1036 M NaOH will be required to reach theequivalence point when 25 mL of the diluted vinegar solutionprepared in part b is titrated?

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