91Ó°ÊÓ

What is the pH of a buffer that is \(0.110 M \mathrm{HPO}_{4}^{2-}\) and \(0.220 M \mathrm{H}_{2} \mathrm{PO}_{4}^{-}\) at \(25^{\circ} \mathrm{C} ?\)

What is the pH of a buffer that is \(0.200 M \mathrm{H}_{2} \mathrm{SO}_{3}\) and \(0.250 \mathrm{M} \mathrm{NaHSO}_{3}\) at \(25^{\circ} \mathrm{C} ?\)

What masses of bromoacetic acid and sodium bromoacetate are needed to prepare \(1.00 \mathrm{L}\) of \(\mathrm{pH}=3.00\) buffer if the total concentration of the two components is \(0.200 M ?\)

What masses of acetic acid and sodium acetate are needed to prepare \(125 \mathrm{mL}\) of \(\mathrm{pH}=5.00\) buffer if the total concentration of the two components is \(0.500 M ?\)

What masses of dimethylamine and dimethylammonium chloride do you need to prepare \(0.500 \mathrm{L}\) of \(\mathrm{pH}=12.00\) buffer if the total concentration of the two components is \(0.300 \mathrm{M} ?\)

What masses of ethylamine and ethylammonium chloride do you need to prepare \(1.00 \mathrm{L}\) of \(\mathrm{pH}=10.50\) buffer if the total concentration of the two components is \(0.250 M ?\)

What is the pH at \(25^{\circ} \mathrm{C}\) of a solution that results from mixing equal volumes of a \(0.05 M\) solution of ammonia and a \(0.025 M\) solution of hydrochloric acid?

What is the pH at \(25^{\circ} \mathrm{C}\) of a solution that results from mixing equal volumes of a \(0.05 M\) solution of acetic acid and a \(0.025 M\) solution of sodium hydroxide?

A buffer consists of \(0.120 \mathrm{MHNO}_{2}\) and \(0.150 \mathrm{MNaNO}_{2}\) at \(25^{\circ} \mathrm{C}\) a. What is the pH of the buffer? b. What is the pH after the addition of \(1.00 \mathrm{mL}\) of \(11.6 \mathrm{M} \mathrm{HCl}\) to \(1.00 \mathrm{L}\) of the buffer solution?

A buffer is prepared by mixing \(50.0 \mathrm{mL}\) of \(0.200 M \mathrm{NaOH}\) with \(100.0 \mathrm{mL}\) of \(0.175 M\) acetic acid. a. What is the pH of the buffer? b. What is the pH of the buffer after \(1.00 \mathrm{g}\) of \(\mathrm{NaOH}\) is dissolved in it?