Question

In: Chemistry

500.0 mL of 0.110 M NaOH is added to 615 mL of 0.200 M weak acid...

500.0 mL of 0.110 M NaOH is added to 615 mL of 0.200 M weak acid (Ka = 7.63

Solutions

Expert Solution

millimoles of acid = 0.2 x 615 =123

millimoles of base = 500 x 0.11=55

HA + NaOH ---------------------------> NaA + H2O

123       55                                       0             0 -----------------------------before reaction

68          0                                        55            55 ------------------------after reaction

in this mixture salt NaA and acid HA remains . it can form buffer

pKa = -log Ka = -log(7.63


Related Solutions

500.0 mL of 0.150 M NaOH is added to 605 mL of 0.200 M weak acid...
500.0 mL of 0.150 M NaOH is added to 605 mL of 0.200 M weak acid (Ka = 5.15 × 10-5). What is the pH of the resulting buffer?
500.0 mL of 0.140 M NaOH is added to 595 mL of 0.200 M weak acid...
500.0 mL of 0.140 M NaOH is added to 595 mL of 0.200 M weak acid (Ka = 2.29 × 10-5). What is the pH of the resulting buffer? HA (aq) + OH (aq) ---> H2O (L) + A (aq)
500.0 mL of 0.140 M NaOH is added to 565 mL of 0.250 M weak acid...
500.0 mL of 0.140 M NaOH is added to 565 mL of 0.250 M weak acid (Ka = 8.39 × 10-5). What is the pH of the resulting buffer? HA(aq)+OH^-(aq)=H2O(l)+ A^-(aq) pH=?
How many mL of 0.200 M NaOH must be added to 100.0 mL of a 0.0500...
How many mL of 0.200 M NaOH must be added to 100.0 mL of a 0.0500 F solution of fumaric acid (transbutenedioic acid) to make a buffer of pH 4.50? Hint: What species do you need in solution to achieve this pH?
A 10.0 mL sample of 0.200 M hydrocyanic acid (HCN) is titrated with 0.0998 M NaOH...
A 10.0 mL sample of 0.200 M hydrocyanic acid (HCN) is titrated with 0.0998 M NaOH . What is the pH at the equivalence point? For hydrocyanic acid, pKa = 9.31.         
A solution is made by mixing exactly 500.0 mL of 0.167 M NaOH with exactly 500.0...
A solution is made by mixing exactly 500.0 mL of 0.167 M NaOH with exactly 500.0 mL of 0.100 M CH3COOH. Calculate the equilibrium concentrations of H3O+, CH3COOH, CH3COO-, OH-, and Na+. [H3O+] = M [CH3COOH] =    M [CH3COO-] =    M [OH-] = M [Na+] = M
The percentage deprotonation of a 0.110 M solution of benzoic acid (a weak, monoprotic acid) is...
The percentage deprotonation of a 0.110 M solution of benzoic acid (a weak, monoprotic acid) is 2.4%. What is the pH of the solution?
If a 0.100 M solution of NaOH is added to a solution containing 0.200 M Ni2+,...
If a 0.100 M solution of NaOH is added to a solution containing 0.200 M Ni2+, 0.200 M Ce3+, and 0.200 M Cu2+, which metal hydroxides will precipitate first and last, respectively? Ksp for Ni(OH)2 is 6.0x10?16, for Ce (OH)3 is 6.0 x 10?22, and for Cu(OH)2 is 4.8x10?20. A) Ni(OH)2 first, Cu(OH)2 last B) Cu(OH)2 first, Ni(OH)2 last C) Ni(OH)2 first, Ce(OH)3 last D) Cu(OH)2 first, Ce(OH)3 last E) Ce(OH)3 first, Cu(OH)2 last Give detailed explanation
Given: 50 ml of 0.2 M weak acid is titrated with 0.2M NaOH. The pka of...
Given: 50 ml of 0.2 M weak acid is titrated with 0.2M NaOH. The pka of the acid is 4.7 1. What is the pH at the equivalence point? 2. What is the ph when 60ml of NaOH is added? (Total Amt of NaOH is 60ml) 3. What is the pH when 10ml of NaOH is added? 4. What would be the approximate ph of a 0.1 M NaCl solution?
Weak acid with strong base: 25 mL of 0.1 M HCOOH with 0.1 M NaOH (pka...
Weak acid with strong base: 25 mL of 0.1 M HCOOH with 0.1 M NaOH (pka = 3.74) pH after adding following amounts of NaOH 18) 0 mL of NaOH 19) at half equivalence point 20) after adding 25 mL NaOH
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT