Consider a buffer solution that contains 0.45 M H3PO4 and 0.55 M NaH2PO4. For H3PO4, Ka1 = 6.9E-3, Ka2 = 6.2E-8, Ka3 = 4.8E-13. Calculate the pH of the buffer solution. Calculate the change in pH if 0.178 g of solid KOH is added to 250 mL of the buffer solution. If the acceptable buffer range is ±0.15 pH units, calculate how many moles of OH- can be neutralized by 207 mL of buffer.
Consider a buffer solution that contains 0.45 M H3PO4 and 0.55 M NaH2PO4. For H3PO4, Ka1 = 6.9E-3, Ka2 = 6.2E-8, Ka3 = 4.8E-13. Calculate the pH of the buffer solution. Calculate the change in pH if 0.178 g of solid KOH is added to 250 mL of the buffer solution. If the acceptable buffer range is ±0.15 pH units, calculate how many moles of OH- can be neutralized by 207 mL of buffer.
Chapter9: Acids, Bases, And Salts
Section: Chapter Questions
Problem 9.102E
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Consider a buffer solution that contains 0.45 M H3PO4 and 0.55 M NaH2PO4. For H3PO4, Ka1 = 6.9E-3, Ka2 = 6.2E-8, Ka3 = 4.8E-13.
Calculate the pH of the buffer solution.
Calculate the change in pH if 0.178 g of solid KOH is added to 250 mL of the buffer solution.
If the acceptable buffer range is ±0.15 pH units, calculate how many moles of OH- can be neutralized by 207 mL of buffer.
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