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Chapter 4: Problem 14

Which of the following must be known to calculate the molarity of a salt solution (there may be more than one answer)? a. the mass of salt added b. the molar mass of the salt c. the volume of water added d. the total volume of the solution Explain

Short Answer

Expert verified
To calculate the molarity of a salt solution, we need to know the mass of salt added (option a), the molar mass of the salt (option b), and the total volume of the solution (option d). Option c, the volume of water added, is not required. The molarity can be calculated using the formula: \(Molarity = \frac{moles\ of\ solute}{volume\ of\ solution\ in\ liters}\).

Step by step solution

01

Analyze Option a – Mass of salt added

The amount of salt added to the solution is needed to calculate the molarity. We need to determine the number of moles of salt, and to do that, we need to know the mass of salt added to the solution. So, option a is required.
02

Analyze Option b – Molar mass of the salt

To determine the moles of solute in the solution, we also need to know the molar mass of the salt. Moles can be calculated by dividing the mass of salt by the molar mass of salt. So, option b is required.
03

Analyze Option c – Volume of water added

The volume of water added to the salt is irrelevant when calculating the molarity. We need to know the total volume of the resulting solution, not just the volume of water added. So, option c is not required.
04

Analyze Option d – Total volume of the solution

Knowing the total volume of the solution is crucial for calculating molarity. As molarity is defined as the number of moles of solute per liter of solution, the total volume of the solution must be known. So, option d is required.
05

Conclusion

Calculating the molarity of a salt solution requires knowing the mass of the salt added (option a), the molar mass of the salt (option b), and the total volume of the solution (option d). The volume of water added (option c) is not needed. Therefore, the correct choices are options a, b, and d.

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Most popular questions from this chapter

For the following chemical reactions, determine the precipitate produced when the two reactants listed below are mixed together. Indicate “none” if no precipitate will form $\mathrm{Sr}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{K}_{3} \mathrm{PO}_{4}(a q) \longrightarrow$__________________(s) $\mathrm{K}_{2} \mathrm{CO}_{3}(a q)+\mathrm{AgNO}_{3}(a q) \longrightarrow$__________________(s) $\mathrm{NaCl}(a q)+\mathrm{KNO}_{3}(a q) \longrightarrow$__________________(s) $\mathrm{KCl}(a q)+\mathrm{AgNO}_{3}(a q) \longrightarrow$__________________(s) $\mathrm{FeCl}_{3}(a q)+\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(a q) \longrightarrow$__________________(s)

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