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Straighterline Chemistry Final- deck 3 Exam
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Straighterline Chemistry Final- deck3 Exam
Which is more soluble in an acidic solution than in pure water?
Select one:
a. CuI
b. PbCl2
c. Ca3(PO4)2
d. NaNO3
e. NaBr - -c. Ca3(PO4)2
-What is the name of the principle of selective precipitation used to identify
the types of ions present in a solution?
Select one:
a. Ionization
b. Selective ion precipitation
c. Selective ion typing
d. Limited precipitation
e. Qualitative analysis - -e. Qualitative analysis
-A 10.0-mL sample of 0.75 M CH3CH2COOH is titrated with 0.30 M NaOH.
What is the pH of the solution after 22.0 mL of NaOH have been added to the
acid?
[Ka(CH3CH2COOH) = 1.3 × 10-5]
Select one:
a. 5.75
b. 4.94
c. 4.83
d. 4.02
e. 3.95 - -a. 5.75
-Methyl red is a common acid-base indicator. It has a Ka equal to 6.3 × 10-6.
Its un-ionized form is red and its anionic form is yellow. What color would a
methyl red solution have at pH = 7.8?
Select one:
a. green
b. red
c. blue
d. yellow
e. violet - -d. yellow
, -A 25.0-mL sample of 0.10 M C2H5NH2 (ethylamine) is titrated with 0.15 M
HCl. What is the pH of the solution after 9.00 mL of acid have been added to
the amine?
[Kb(C2H5NH2) = 6.5 × 10-4]
Select one:
a. 11.08
b. 10.74
c. 10.81
d. 10.55
e. 10.49 - -b. 10.74
-A 35.0-mL sample of 0.20 M LiOH is titrated with 0.25 M HCl. What is the pH
of the solution after 23.0 mL of HCl have been added to the base?
Select one:
a. 1.26
b. 1.67
c. 12.33
d. 12.74
e. 13.03 - -c. 12.33
-A 25.0-mL sample of 1.00 M NH3 is titrated with 0.15 M HCl. What is the pH
of the solution after 15.00 mL of acid have been added to the ammonia
solution?
[Kb(NH3) = 1.8 × 10-5]
Select one:
a. 10.26
b. 9.30
c. 9.21
d. 8.30
e. 8.21 - -a. 10.26
-When a strong acid is titrated with a weak base, the pH at the equivalence
point
Select one:
a. is greater than 7.0.
b. is equal to 7.0.
c. is less than 7.0.
d. is equal to the pKa of the conjugate acid.
e. is equal to the pKb of the base. - -c. is less than 7.0.
-A buffer is prepared by adding 300.0 mL of 2.0 M NaOH to 500.0 mL of 2.0
M CH3COOH. What is the pH of this buffer? [Ka(CH3COOH) = 1.8 × 10-5]
Select one:
a. 4.57
b. 4.52
c. 4.87
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