For the following questions, wherever is necessary write the chemical equation(s) (pay tention to arrow(s) direction), mass balance equation(s) and then show all your assumption(s) and finally do not forget to verify assumption(s). Formic acid is a weak acid with molecular formula of HCOOH (represent as HA). K, for formic acid (HA)=1.8x10“. M.W. for formic acid= 46.03 g/mol, for sodium formate= 68.01 g/mol a) What is the pH of 0.300 M formic acid solution? b) What would be the pH of solution if 100.0 ml of 0.300 M formic acid is mixed 100.0 mL of 0.100 M NaOH solution? c) What mass of sodium formate (NACOOH, represent as NaA) must be added to 100.0 mL of 0.300 M formic acid to produce a buffer solution with a pH of 4.00?
For the following questions, wherever is necessary write the chemical equation(s) (pay tention to arrow(s) direction), mass balance equation(s) and then show all your assumption(s) and finally do not forget to verify assumption(s). Formic acid is a weak acid with molecular formula of HCOOH (represent as HA). K, for formic acid (HA)=1.8x10“. M.W. for formic acid= 46.03 g/mol, for sodium formate= 68.01 g/mol a) What is the pH of 0.300 M formic acid solution? b) What would be the pH of solution if 100.0 ml of 0.300 M formic acid is mixed 100.0 mL of 0.100 M NaOH solution? c) What mass of sodium formate (NACOOH, represent as NaA) must be added to 100.0 mL of 0.300 M formic acid to produce a buffer solution with a pH of 4.00?
Chemistry: The Molecular Science
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Chapter10: Fuels, Organic Chemicals, And Polymers
Section10.2: U. S/ Energy Sources And Consumption
Problem 10.4E
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Transcribed Image Text:For the following questions, wherever is necessary write the chemical equation(s) (pay attention
to arrow(s) direction), mass balance equation(s) and then show all your assumption(s) and finally do not
forget to verify assumption(s).
Formic acid is a weak acid with molecular formula of HCOOH (represent as HA).
K, for formic acid (HA)=1.8x10ª.
M.W. for formic acid= 46.03 g/mol, for sodium formate= 68.01 g/mol
a) What is the pH of 0.300 M formic acid solution?
b) What would be the pH of solution if 100.0 mL of 0.300 M formic acid is mixed 100.0 ml of 0.100 M NaOH
solution?
c) What mass of sodium formate (NacOOH, represent as NaA) must be added to 100.0 ml of 0.300 M formic
acid to produce a buffer solution with a pH of 4.00?
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