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Determine the pH at the point in the titration of 40.0 mL of 0.200 M HC₄H₇O₂ with 0.100 M Sr(OH)₂ after 100.0 mL of the strong base has been added. The value of Ka for HC₄H₇O₂ is 1.5 × 10⁻⁵. Is my ICE table correct? if not can you help me correct it by creating an ICE TABLE? and determine the pH base on the result of the acid-base reaction? thank you!

Determine the pH at the point in the titration of 40.0 mL of 0.200 M HC₄H₇O₂ with 0.100 M Sr(OH)₂ after 100.0 mL of the strong base has been added. The value of Ka for HC₄H₇O₂ is 1.5 × 10⁻⁵. Is my ICE table correct? if not can you help me correct it by creating an ICE TABLE? and determine the pH base on the result of the acid-base reaction? thank you!

Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Determine the pH at the point in the titration of 40.0 mL of 0.200 M HC₄H₇O₂ with 0.100 M Sr(OH)₂ after 100.0 mL of the strong base has been added. The value of Ka for HC₄H₇O₂ is 1.5 × 10⁻⁵. Is my ICE table correct? if not can you help me correct it by creating an ICE TABLE? and determine the pH base on the result of the acid-base reaction? thank you!

**Chemical Reaction Table** Use the table below to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of liquid water in the reaction. | | HC₄H₇O₂(aq) | + | OH⁻(aq) | → | H₂O(l) | + | C₄H₇O₂⁻(aq) | |-------|-------------|---|--------|---|-------|---|-------------| | Before (mol) | 8.00 × 10⁻³ | | 2.00 × 10⁻² | | | | 0 | | Change (mol) | −8.00 × 10⁻³ | | −2.00 × 10⁻³ | | | | 8.00 × 10⁻³ | | After (mol) | 0 | | 1.20 × 10⁻² | | | | 8.00 × 10⁻³ | **Explanation:** - **Before the Reaction:** - HC₄H₇O₂(aq): 8.00 × 10⁻³ moles - OH⁻(aq): 2.00 × 10⁻² moles - C₄H₇O₂⁻(aq): 0 moles - **Change during the Reaction:** - HC₄H₇O₂(aq) and OH⁻(aq) both decrease as they react, with changes of −8.00 × 10⁻³ and −2.00 × 10⁻³ moles, respectively. - C₄H₇O₂⁻(aq) is produced, increasing by 8.00 × 10⁻³ moles. - **After the Reaction:** - HC₄H₇O₂(aq): 0 moles (completely reacted) - OH⁻(aq): 1.20 × 10⁻² moles remain - C₄H₇O₂⁻(aq): 8.00 × 10⁻³ moles formed as product Note: The table does not account for the moles
Transcribed Image Text:**Chemical Reaction Table** Use the table below to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of liquid water in the reaction. | | HC₄H₇O₂(aq) | + | OH⁻(aq) | → | H₂O(l) | + | C₄H₇O₂⁻(aq) | |-------|-------------|---|--------|---|-------|---|-------------| | Before (mol) | 8.00 × 10⁻³ | | 2.00 × 10⁻² | | | | 0 | | Change (mol) | −8.00 × 10⁻³ | | −2.00 × 10⁻³ | | | | 8.00 × 10⁻³ | | After (mol) | 0 | | 1.20 × 10⁻² | | | | 8.00 × 10⁻³ | **Explanation:** - **Before the Reaction:** - HC₄H₇O₂(aq): 8.00 × 10⁻³ moles - OH⁻(aq): 2.00 × 10⁻² moles - C₄H₇O₂⁻(aq): 0 moles - **Change during the Reaction:** - HC₄H₇O₂(aq) and OH⁻(aq) both decrease as they react, with changes of −8.00 × 10⁻³ and −2.00 × 10⁻³ moles, respectively. - C₄H₇O₂⁻(aq) is produced, increasing by 8.00 × 10⁻³ moles. - **After the Reaction:** - HC₄H₇O₂(aq): 0 moles (completely reacted) - OH⁻(aq): 1.20 × 10⁻² moles remain - C₄H₇O₂⁻(aq): 8.00 × 10⁻³ moles formed as product Note: The table does not account for the moles
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