1 answer

A chemistry graduate student is given 500.mL of a 0.70M chloroacetic acid HCH2ClCO2 solution. Chloroacetic acid...

Question:

A chemistry graduate student is given 500.mL of a 0.70M chloroacetic acid HCH2ClCO2 solution. Chloroacetic acid is a weak acid with =Ka×1.310−3. What mass of NaCH2ClCO2 should the student dissolve in the HCH2ClCO2 solution to turn it into a buffer with pH =3.40? You may assume that the volume of the solution doesn't change when the NaCH2ClCO2 is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.


Answers

Given =) ka for HCH2C1602 = 1.3x10-3 concentration of HCH2C1C02 = 0.70m . pH=3.40 we know that pH of acidic buffer pH e praf(NaCH₂ C1 (O2) = 3: 266 0.70m. [na CH2 C1002]- 3.266X0.70M (NO CH2C1CO2 = 2:2862 m No. of mol of NacHa alco2 = Molarity x vol

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