1. Which solution has the lowest pH?
A. 0.10 M HClO4
B. 0.10 M HClO
C. 0.10 M KOH
D. 0.10 M CH3NH2
2. Which solution has the highest pH?
A. 0.05 M Sr(OH)2
B. 0.10 M Sr(OH)2
C. 0.10 M NaOH
D. 0.15 M NaOH
3. What is the pH of 0.03 M acid solution? The Ka of the acid is 510-3?
A. 1.5
B. 1.9
C. 2.0
D. 2.3
4. What is the pH of 0.10 M Ba(OH)2 solution?
A. 0.70
B. 1.00
C. 13.00
D. 13.30
5. What is the [OH- ] of a solution with pH = 4.33?
A. 2.1104 M
B. 2.110-10 M
C. 4.7109 M
D. 4.710-5 M
6. A 0.025 M solution of compound X has pH = 2.15. Which of the following statements is true?
A. Compound X is a strong acid.
B. Compound X is a strong base.
C. Compound X is a weak acid.
D. Compound X is a weak base.
7. A base has % ionization of 0.3%. What is the pH of 0.05 M solution of the base?
A. 1.3
B. 3.8
C. 10.2
D. 12.7
1- "0.10MHCLO_4" has the lowest PH.
2- Ph of base ="pOH=-log(OH)"
then pH "=14-pOH"
3-"[H^+]= {K_aC}^\\dfrac{1}{2}"
then pH ="-log(H^+)"
4- "[OH^-]={K_bC}^\\dfrac{1}{2}"
then pOH="-log(OH)"
Now pH ="14-pOH"
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