Questions: Question 2 (6 points) What is the pH of a solution if there are 0.00258 grams of H+ present in 1 L of this solution? Round your answer to one decimal place. Question 3 (6 points) You have two solutions, A and B, separated by a semipermeable membrane. Solution A is 0.5 moles of KCl in 1 LH2O and Solution B is 0.8 moles of dextrose in 1 LH2O. Which side has the higher osmotic pressure at 25°C and what is that pressure? Enter the letter solution with the higher pressure as the Unit. Question 4 (6 points) Over the course of 12 minutes a reaction uses up 120 grams of the reactant Hif. What is the rate of

What is the pH of a solution if there are 0.00258 grams of \(\mathrm{H}^{+}\) present in 1 L of this solution? Round your answer to one decimal place.

Calculate the number of moles of \(\mathrm{H}^{+}\)

The molar mass of \(\mathrm{H}^{+}\) is approximately 1 g/mol. Therefore, the number of moles of \(\mathrm{H}^{+}\) is: \[ \text{moles of } \mathrm{H}^{+} = \frac{0.00258 \text{ grams}}{1 \text{ g/mol}} = 0.00258 \text{ moles} \]

Calculate the concentration of \(\mathrm{H}^{+}\)

Since the solution volume is 1 L, the concentration of \(\mathrm{H}^{+}\) is: \[ [\mathrm{H}^{+}] = \frac{0.00258 \text{ moles}}{1 \text{ L}} = 0.00258 \text{ M} \]

Calculate the pH

The pH is calculated using the formula: \[ \text{pH} = -\log [\mathrm{H}^{+}] \] Substituting the concentration: \[ \text{pH} = -\log (0.00258) \approx 2.6 \]

\(\boxed{2.6}\)

You have two solutions, \(A\) and \(B\), separated by a semipermeable membrane. Solution \(A\) is 0.5 moles of KCl in 1 L of \(\mathrm{H}_{2}\mathrm{O}\) and Solution \(B\) is 0.8 moles of dextrose in 1 L of \(\mathrm{H}_{2}\mathrm{O}\). Which side has the higher osmotic pressure at \(25^{\circ} \mathrm{C}\) and what is that pressure? Enter the letter solution with the higher pressure as the Unit.

Calculate the osmotic pressure of Solution \(A\)

The osmotic pressure \(\Pi\) is given by the formula: \[ \Pi = iMRT \] For KCl, \(i = 2\) (since KCl dissociates into \(K^{+}\) and \(Cl^{-}\)). Therefore: \[ \Pi_A = 2 \times 0.5 \text{ M} \times 0.0821 \text{ L atm K}^{-1} \text{ mol}^{-1} \times 298 \text{ K} = 24.5 \text{ atm} \]

Calculate the osmotic pressure of Solution \(B\)

For dextrose, \(i = 1\) (since it does not dissociate). Therefore: \[ \Pi_B = 1 \times 0.8 \text{ M} \times 0.0821 \text{ L atm K}^{-1} \text{ mol}^{-1} \times 298 \text{ K} = 19.6 \text{ atm} \]

Determine which solution has the higher osmotic pressure

Comparing the osmotic pressures: \[ \Pi_A = 24.5 \text{ atm} \quad \text{and} \quad \Pi_B = 19.6 \text{ atm} \] Solution \(A\) has the higher osmotic pressure.

\(\boxed{A}\) \(\boxed{24.5 \text{ atm}}\)

\(\boxed{2.6}\)

\(\boxed{A}\) \(\boxed{24.5 \text{ atm}}\)