0.250 M NaOH is used to titrate 20.0 mL of 0.15 M HCO2H (Ka=1.8x10^-4). What is the pH after the addition of 8.00 mL of of NaOH?
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1. ) Calculate the pH for a buffer solution prepared by mixing 100.0mL of 0.10M HF and 200.0mL of 0.10M KF. Ka = 6.6 x 10-4
2.)0.2 M NaOH is used to titrate 20 mL of 0.1 M HCl. a) What is the volume, in mL, of NaOH needed to reach the equivalence point? (Do not include units and round a whole number) b) What is the pH at this point?
3.)0.2 M NaOH is used to titrate 20 mL of 0.1 M HCl. What is the pH when 6 mL of the NaOH is added?
4.) 0.2 M NaOH is used to titrate 20 mL of 0.1 M HCl. What is the pH when 18 mL of the NaOH is added?
5.)Calculate the pH of a 0.35 M solution of NH3. The Kb for NH3 is 1.8x10-5.
a total volume of 33.15 ml of naoh is needed to titrate 24.5 ml of .1053 m acetic acid ( ka= 1.8x10^-5) to the equivalence point. what is the ph at the equivalence point ?
Help please!
A 30.0-mL volume of 0.50 M CH3COOH (Ka=1.8x10^-5) was titratedwith 0.50 M NaOH. Calculate the pH after addition of 30.0 mL ofNaOH