Given a solution containing 2.00 × 10^{-3} M Ca^{2+} and 3.00 × 10^{-2} M SO_4^{2-}, what is the value of the charge (q) carried by the ions in 1.00 L of this solution? (Use the elementary charge e = 1.602 × 10^{-19} C.)

• A. q = 9.61 × 10^{1} C
• B. q = 1.28 × 10^{2} C
• C. q = 1.60 × 10^{1} C
• D. q = 3.20 × 10^{0} C

Answer: (C)

Verified step by step guidance

1. Identify the ions present in the solution and their concentrations: Ca^{2+} with concentration 2.00 \times 10^{-3} M and SO_4^{2-} with concentration 3.00 \times 10^{-2} M.
2. Calculate the number of moles of each ion in 1.00 L of solution by using the formula: moles = concentration (M) \times volume (L). Since the volume is 1.00 L, the moles equal the concentration values directly.
3. Determine the total number of ions for each species by multiplying the moles by Avogadro's number (N_A = 6.022 \times 10^{23} ions/mol): Number of ions = moles \times N_A.
4. Calculate the total charge contributed by each ion type using the formula: Charge (C) = number of ions \times charge per ion \times elementary charge (e), where the charge per ion is the magnitude of the ion's charge (2 for Ca^{2+} and SO_4^{2-}), and e = 1.602 \times 10^{-19} C.
5. Sum the charges from both ion types to find the total charge q carried by the ions in 1.00 L of solution.