Question
The $\mathrm{pH}$ of $0.005 \mathrm{M}-\mathrm{NaOH}$ solution is $(\log 2=0.3)$(a) $2.3$(b) $2.7$(c) $11.3$(d) $11.7$
Step 1
005 \, \text{M}$ to $5 \times 10^{-3} \, \text{M}$ for easier calculation. Show more…
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$$ \begin{aligned} &\mathrm{NaOH} \text { is a strong base. What will be } \mathrm{pH} \text { of } 5.0 \times 10^{-2} \mathrm{M} \mathrm{NaOH}\\ &\text { solution ? }(\log 2=0.3) \end{aligned} $$ (a) $14.00$ (b) $13.70$ (c) $13.00$ (d) $12.70$
Equilibrium
Topic 2 : Ionic Equilibrium
What is the pH of a 0.005 M solution of NaOH (aq)? a. 11.7 b. 12 c. 12.3 d. 13
The $\mathrm{pH}$ of $0.001 \mathrm{~N}$ sodium hydroxide solution at $25^{\circ} \mathrm{C}$ is (a) 3 (b) 4 (c) 11 (d) 12
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