1.What is the pH of 0.15 M HI and the pH of 0.15 M H 2 S? 2. An example of P in
ID: 905763 • Letter: 1
Question
1.What is the pH of 0.15 M HI and the pH of 0.15 M H2S?
2. An example of P in its maximum and minimum oxidation states is:
a)white phosphorus and red phosphorus
b)P4O10 and PH3
c)H3PO4 and Na3PO4
d)PH3 and Na3P
3.Match the following statements in Column A with the correct answer from Column B
A B
Formed when hydrochloric acid reacts with sodium hydroxide O2
Formed when potassium peroxide is heated N2
Formed when ammonium chloride is heated Cl2
Formed when calcium hypochlorite reacts with HCl CH3COOH
Formed when sodium oxide reacts with water HCl
H2
NaOH
NaCl
Explanation / Answer
1) pH of 0.15 M HI :
[H+] = 0.15 N (For monoprotic acids, Molarity and normality are equal)
pH = -log [H+]
= - log [0.15]
= 0.823
pH = 0.823
pH of 0.15 M H2S
[H+] = 0.15 M = 0.15x 2 N = 0.30 N ( For diprotic acids, Normality = Molarity x 2)
pH = -log [H+]
= - log [0.30]
= 0.522
pH = 0.522
2)
An example of P in its maximum and minimum oxidation states is:
a)white phosphorus and red phosphorus b)P4O10 and PH3 c)H3PO4 and Na3PO4 d)PH3 and Na3P
Ans : b
Maximum oxidation state of P is +5 and minimum oxidation state is -3.
a) white phosphorus and red phosphorus
In both, oxidation state of P = 0
b) P4O10 and PH3
P4O10 : 4P+ 10 (-2) = 0
P = +5
PH3 : P + 3(+1) = 0
P = -3
c) H3PO4 and Na3PO4
H3PO4 : 3(+1) + P + 4(-2) = 0
P = +5
Na3PO4 :
3(+1) + P + 4(-2) = 0
P = +5
d) PH3 and Na3P
PH3 : P + 3(+1) = 0
P = -3
Na3P : 3(+1) + P = 0
P = -3
3) a) when hydrochloric acid reacts with sodium hydroxide = NaCl will be formed
HCl + NaOH ----------> NaCl + H2O
b) when potassium peroxide is heated = O2 will be formed
2 K2O2 ------> 2 K2O + O2
c) when ammonium chloride is heated = HCl will be formed
NH4Cl -------------> NH3+HCl
d) when calcium hypochlorite reacts with HCl = Cl2 wil be formed
Ca(OCl)2 + 4 HCl ------------------> CaCl2 + 2 H2O + 2 Cl2
e)when sodium oxide reacts with water = NaOH will be formed.
Na2O + H2O -------------> 2 NaOH
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