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Asked Mar 24, 2019
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Important equations
[H+] [OH-] = Kw = 1.00 X 10-14 (at 25 °C)
pH =-log [H+] pOH =-log [OH-]
pH + pOH = 14.00
H I[A
[HA]
Classify the following as either acidic, basic or neutral.
1.
a. NaCl
b. NH4Cl
c. KNO2
d. NaF
e. KNO3
f. NH4NO3
g. KC2H302
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Important equations [H+] [OH-] = Kw = 1.00 X 10-14 (at 25 °C) pH =-log [H+] pOH =-log [OH-] pH + pOH = 14.00 H I[A [HA] Classify the following as either acidic, basic or neutral. 1. a. NaCl b. NH4Cl c. KNO2 d. NaF e. KNO3 f. NH4NO3 g. KC2H302

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Step 1

a.

Neutral salts - NaCl

Because the neutralization reaction of strong acid (HCl) and strong base (NaOH)

Step 2

b.

Acidic salts – NH4Cl

Because the neutralization reaction of strong acid (HCl) and weak base (NH4OH)

Step 3

c.

Basic salts - KNO2

Because the neutralization reaction of weak ...

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