Write a balanced net ionic equation for the neutralization of equimolar amounts of H N O 2 and KOH. Indicate whether the pH after neutralization is greater than, equal to, or less than 7. Values of K a and K B are listed in Appendix C.
Write a balanced net ionic equation for the neutralization of equimolar amounts of H N O 2 and KOH. Indicate whether the pH after neutralization is greater than, equal to, or less than 7. Values of K a and K B are listed in Appendix C.
Write a balanced net ionic equation for the neutralization of equimolar amounts of
H
N
O
2
and KOH. Indicate whether the pH after neutralization is greater than, equal to, or less than 7. Values of
K
a
and
K
B
are listed in Appendix C.
Expert Solution & Answer
Interpretation Introduction
Interpretation:
A balance net ionic equation for the neutralization of equimolar amount of HNO2 and KOH needs to be determined, if the pH after neutralization is greater than, equal to or less than 7 needs to be determined.
Concept introduction:
In the balance equation number of atoms of particular element i.e reactant is equals to number of atoms of that element as a product.
pH is a measure of hydrogen ion concentration. It expresses the acidity and basicity of a solution.
Answer to Problem 17.1P
HNO2(aq)+OH−(aq)→NO2−(aq)+H2O(l)
After neutralization, pH is greater than 7 for the given equation.
Explanation of Solution
HNO2 is a week acid and KOH is a strong base. The balance net ionic equation for the neutralization of equimolar amounts of HNO2 and KOH is as follows:
HNO2(aq)+OH−(aq)→NO2−(aq)+H2O(l)
The solution contains NO2− weak base and K+ ion after neutralization. Thus pH is greater than 7.
Conclusion
Thus, the balanced chemical equation is as follows:
HNO2(aq)+OH−(aq)→NO2−(aq)+H2O(l)
After neutralization, pH is greater than 7 for the given equation.
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