229829 $20 \mathrm{~mL}$ of $0.1 \mathrm{M}$ acetic acid is mixed in a solution of $\mathrm{NaOH}$. If $10 \mathrm{~mL}$ of $0.1 \mathrm{M} \mathrm{NaOH}$ is present then $\mathrm{H}^{+}$concentration in resulting solution is $\left(\mathrm{K}_{\mathrm{a}}\right.$ of acetic acid $=1.7 \times 10^{-5}$ )

229830 Which of the following have maximum $\mathrm{pH}$ ?

229831 $\mathrm{K}_{\text {sp }}$ of $\mathrm{M}(\mathrm{OH})_2$ is $3.2 \times 10^{-11}$. The $\mathrm{pH}$ of saturated solution in water is

229835 $40 \mathrm{~mL}$ of $0.1 \mathrm{M}$ ammonia solution is mixed with $40 \mathrm{~mL}$ of $0.1 \mathrm{MHCl}$. What is the $\mathrm{pH}$ of the mixture? (pK $\mathrm{pK}_{\mathrm{b}}$ of ammonia solution is 4.74).

229836 When $10 \mathrm{~mL}$ of $0.1 \mathrm{M}$ acetic acid $\left(\mathrm{pK}_{\mathrm{a}}=5.0\right)$, is titrated against $10 \mathrm{~mL}$ of $0.1 \mathrm{M}$ ammonia solution $\left(\mathrm{pK}_{\mathrm{b}}=5.0\right)$, the equivalence point occurs at $\mathrm{pH}$ :

229829 $20 \mathrm{~mL}$ of $0.1 \mathrm{M}$ acetic acid is mixed in a solution of $\mathrm{NaOH}$. If $10 \mathrm{~mL}$ of $0.1 \mathrm{M} \mathrm{NaOH}$ is present then $\mathrm{H}^{+}$concentration in resulting solution is $\left(\mathrm{K}_{\mathrm{a}}\right.$ of acetic acid $=1.7 \times 10^{-5}$ )

229830 Which of the following have maximum $\mathrm{pH}$ ?

229831 $\mathrm{K}_{\text {sp }}$ of $\mathrm{M}(\mathrm{OH})_2$ is $3.2 \times 10^{-11}$. The $\mathrm{pH}$ of saturated solution in water is

229835 $40 \mathrm{~mL}$ of $0.1 \mathrm{M}$ ammonia solution is mixed with $40 \mathrm{~mL}$ of $0.1 \mathrm{MHCl}$. What is the $\mathrm{pH}$ of the mixture? (pK $\mathrm{pK}_{\mathrm{b}}$ of ammonia solution is 4.74).

229836 When $10 \mathrm{~mL}$ of $0.1 \mathrm{M}$ acetic acid $\left(\mathrm{pK}_{\mathrm{a}}=5.0\right)$, is titrated against $10 \mathrm{~mL}$ of $0.1 \mathrm{M}$ ammonia solution $\left(\mathrm{pK}_{\mathrm{b}}=5.0\right)$, the equivalence point occurs at $\mathrm{pH}$ :

229829 $20 \mathrm{~mL}$ of $0.1 \mathrm{M}$ acetic acid is mixed in a solution of $\mathrm{NaOH}$. If $10 \mathrm{~mL}$ of $0.1 \mathrm{M} \mathrm{NaOH}$ is present then $\mathrm{H}^{+}$concentration in resulting solution is $\left(\mathrm{K}_{\mathrm{a}}\right.$ of acetic acid $=1.7 \times 10^{-5}$ )

229830 Which of the following have maximum $\mathrm{pH}$ ?

229831 $\mathrm{K}_{\text {sp }}$ of $\mathrm{M}(\mathrm{OH})_2$ is $3.2 \times 10^{-11}$. The $\mathrm{pH}$ of saturated solution in water is

229835 $40 \mathrm{~mL}$ of $0.1 \mathrm{M}$ ammonia solution is mixed with $40 \mathrm{~mL}$ of $0.1 \mathrm{MHCl}$. What is the $\mathrm{pH}$ of the mixture? (pK $\mathrm{pK}_{\mathrm{b}}$ of ammonia solution is 4.74).

229836 When $10 \mathrm{~mL}$ of $0.1 \mathrm{M}$ acetic acid $\left(\mathrm{pK}_{\mathrm{a}}=5.0\right)$, is titrated against $10 \mathrm{~mL}$ of $0.1 \mathrm{M}$ ammonia solution $\left(\mathrm{pK}_{\mathrm{b}}=5.0\right)$, the equivalence point occurs at $\mathrm{pH}$ :

229829 $20 \mathrm{~mL}$ of $0.1 \mathrm{M}$ acetic acid is mixed in a solution of $\mathrm{NaOH}$. If $10 \mathrm{~mL}$ of $0.1 \mathrm{M} \mathrm{NaOH}$ is present then $\mathrm{H}^{+}$concentration in resulting solution is $\left(\mathrm{K}_{\mathrm{a}}\right.$ of acetic acid $=1.7 \times 10^{-5}$ )

229830 Which of the following have maximum $\mathrm{pH}$ ?

229831 $\mathrm{K}_{\text {sp }}$ of $\mathrm{M}(\mathrm{OH})_2$ is $3.2 \times 10^{-11}$. The $\mathrm{pH}$ of saturated solution in water is

229835 $40 \mathrm{~mL}$ of $0.1 \mathrm{M}$ ammonia solution is mixed with $40 \mathrm{~mL}$ of $0.1 \mathrm{MHCl}$. What is the $\mathrm{pH}$ of the mixture? (pK $\mathrm{pK}_{\mathrm{b}}$ of ammonia solution is 4.74).

229836 When $10 \mathrm{~mL}$ of $0.1 \mathrm{M}$ acetic acid $\left(\mathrm{pK}_{\mathrm{a}}=5.0\right)$, is titrated against $10 \mathrm{~mL}$ of $0.1 \mathrm{M}$ ammonia solution $\left(\mathrm{pK}_{\mathrm{b}}=5.0\right)$, the equivalence point occurs at $\mathrm{pH}$ :

229829 $20 \mathrm{~mL}$ of $0.1 \mathrm{M}$ acetic acid is mixed in a solution of $\mathrm{NaOH}$. If $10 \mathrm{~mL}$ of $0.1 \mathrm{M} \mathrm{NaOH}$ is present then $\mathrm{H}^{+}$concentration in resulting solution is $\left(\mathrm{K}_{\mathrm{a}}\right.$ of acetic acid $=1.7 \times 10^{-5}$ )

229830 Which of the following have maximum $\mathrm{pH}$ ?

229831 $\mathrm{K}_{\text {sp }}$ of $\mathrm{M}(\mathrm{OH})_2$ is $3.2 \times 10^{-11}$. The $\mathrm{pH}$ of saturated solution in water is

229835 $40 \mathrm{~mL}$ of $0.1 \mathrm{M}$ ammonia solution is mixed with $40 \mathrm{~mL}$ of $0.1 \mathrm{MHCl}$. What is the $\mathrm{pH}$ of the mixture? (pK $\mathrm{pK}_{\mathrm{b}}$ of ammonia solution is 4.74).

229836 When $10 \mathrm{~mL}$ of $0.1 \mathrm{M}$ acetic acid $\left(\mathrm{pK}_{\mathrm{a}}=5.0\right)$, is titrated against $10 \mathrm{~mL}$ of $0.1 \mathrm{M}$ ammonia solution $\left(\mathrm{pK}_{\mathrm{b}}=5.0\right)$, the equivalence point occurs at $\mathrm{pH}$ :