1.Calculate the pH of each solution: a)1.55 x 10-2 M HBr b) 2.28 x 10-3 M KOH c)
ID: 994634 • Letter: 1
Question
1.Calculate the pH of each solution:
a)1.55 x 10-2 M HBr
b) 2.28 x 10-3 M KOH
c)8.89 x 10-3 M HNO3
d) 6.54 x 10-4 M Sr(OH)2
2. A buffer contains HCHO2 (aq) and KCHO2 (aq). Which statement correctly summarizes the action of this buffer?
a)HCHO2 (aq) neutralizes added acid, and KCHO2 (aq) neutralizes added base.
b)HCHO2 (aq neutalizes added base, and KCHO2 (aq) neutalizes added acid.
c)Both HCHO2 (aq) and KCHO2 (aq) neutalize added acid.
d) Both HCHO2 (aq) and KCHO2 (aq) neutralizes added base
3. What substance could you add to each solution to make it a buffer solution?
a) 0.050 M NaHSO3
b) 0.150 M HF
c) 0.200 M KCHO2
4. Write a reaction showing how HC2H3O2 and NaC2H3O2 buffer would neutralize added NaOH.
5. Determine which of the mistures is a buffer
a) HCHO2 and NaCHO2
b) HCl and HBr
c)HBr and NaCl
d)KOH and NH3
6. A 0.105g sample of a monoprotic acid of unknown molar mass is dissolved in water and titrated with 0.1003 M NaOH. The equivalence point is reached after adding 28.68 ml of base. What is the molar mass of the unknown acid?
Explanation / Answer
1.Calculate the pH of each solution:
a)1.55 x 10-2 M HBr
pH = -log(H+)
pH = -log( 1.55*10^-2)
pH = 1.8096
b) 2.28 x 10-3 M KOH
pOH = -log(OH) = -log(2.28*10^-3)
pH = 14-2.64206 = 11.357
c)8.89 x 10-3 M HNO3
pH = -loG(H)
pH = -log(8.89*10^-3) =2.051098
d) 6.54 x 10-4 M Sr(OH)2
pO H= -log(OH)
OH = 2*6.54*10^-4) = 0.001308
pOH = -log(0.001308) =2.883
pH = 14-2.883 = 11.117
NOTE Consider posting multiple questions in mutliple set of Q&A.
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