What is the $pH$ of a solution in which $25.0 \ mL$ of $0.1 \ M \ NaOH$ is added to $25 \ mL$ of $0.08 \ M \ HCl$ and the final solution is diluted to $500 \ mL$?
- A$3$
- B$11$
- C$12$
- D$13$
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Calculate the $pH$ of the following solutions:
$(a)$ $0.1 \ M \ HCl$
$(b)$ $0.1 \ M \ H_2SO_4$
$(c)$ $0.1 \ M \ HNO_3$
$(d)$ $0.1 \ M \ NaOH$
$(e)$ $0.1 \ M \ KOH$
$(f)$ $0.1 \ M \ Ba(OH)_2$
$(a)$ $0.1 \ M \ HCl$
$(b)$ $0.1 \ M \ H_2SO_4$
$(c)$ $0.1 \ M \ HNO_3$
$(d)$ $0.1 \ M \ NaOH$
$(e)$ $0.1 \ M \ KOH$
$(f)$ $0.1 \ M \ Ba(OH)_2$
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