1.What is the pH of a solution that has [OH - ] = 4.0 ´ 10 9 M ? 8.40 5.60 4.60
ID: 103087 • Letter: 1
Question
1.What is the pH of a solution that has [OH-] = 4.0 ´ 109 M?
8.40
5.60
4.60
9.40
none of these
2.Choose the case that is not a conjugate acid-base pair.
H3O+, H2O
H3PO4, HPO42-
OH-, O2
NH2OH2+, NH2OH
HCO3-, CO32
3.Calculate the [H+] in a solution that has a pH of 5.21.
1.6 ´ 109 M
6.2 ´ 106 M
4.0 ´ 103 M
1.6 ´ 102 M
none of these
4.A 51.24-g sample of Ba(OH)2 is dissolved in enough water to make 1.20 L of solution. How many milliliters of this solution must be diluted with water in order to make 1.00 L of 0.100 M Ba(OH)2?
1.20 ´ 103 mL
400. mL
278 mL
333 mL
none of these
5.How many grams of NaCl are contained in 350. mL of a 0.250 M solution of sodium chloride?
5.11 g
87.5 g
14.6 g
41.7 g
none of these
a.8.40
b.5.60
c.4.60
d.9.40
e.none of these
Explanation / Answer
1)
we have below equation to be used:
pOH = -log [OH-]
= -log (4*10^-9)
= 8.40
we have below equation to be used:
PH = 14 - pOH
= 14 - 8.40
= 5.60
Answer: b
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