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Chapter 4: Problem 13

You have two solutions of chemical A. To determine which has the highest concentration of A (molarity), which of the following must you know (there may be more than one answer)? a. the mass in grams of A in each solution b. the molar mass of A c. the volume of water added to each solution d. the total volume of the solution Explain.

Short Answer

Expert verified
To determine which solution has the highest concentration (molarity) of chemical A, you need to know: - the mass in grams of A in each solution (Option a) - the molar mass of A (Option b) - the total volume of the solution (Option d) Option c (the volume of water added) is not necessary.

Step by step solution

01

Molarity Formula

Molarity (M) is the number of moles of solute (in our case, chemical A) per liter of solution. The formula to calculate molarity is: M = moles of solute / liters of solution Therefore, to compare the molarity of the two solutions, we must know: 1. The number of moles of chemical A in each solution 2. The total volume of each solution Now, let's analyze each option to see if they provide the required information to calculate molarity.
02

Option a: mass in grams

Knowing the mass in grams of chemical A in each solution does not directly provide the number of moles. However, it is related and can be used in combination with the molar mass (Option b) to find the number of moles. Without the molar mass, Option a alone does not provide enough information to calculate molarity.
03

Option b: molar mass

The molar mass of a substance is the mass of one mole of that substance. This information helps us convert the mass of chemical A in grams (Option a) to the number of moles. Thus, the molar mass is necessary for calculating molarity when given the mass of the solute, but it is not sufficient on its own.
04

Option c: volume of water added

Knowing the volume of water added to each solution does not provide enough information to find the total volume of the solution, as it only considers the solvent (water) and not the solute (chemical A). Therefore, this option alone is not enough to calculate molarity.
05

Option d: total volume of the solution

The total volume of the solution is an essential factor for calculating molarity, as it is needed in the denominator of the molarity formula. This option, when combined with the number of moles of the solute or the information required to obtain it (Options a and b), allows us to calculate molarity.
06

Conclusion

To find out which solution has the highest concentration (molarity) of chemical A, we need to know: - the mass in grams of A in each solution (Option a) - the molar mass of A (Option b) - the total volume of the solution (Option d) Therefore, the correct answers are a, b, and d. Option c (the volume of water added) is not necessary to determine which solution has the highest molarity of chemical A.

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Most popular questions from this chapter

Assign the oxidation state for the element listed in each of the following compounds: \(\mathrm{S}\) in \(\mathrm{MgSO}_{4}\)_______ \(\mathrm{Pb}\) in \(\mathrm{PbSO}_{4}\)______ \(\mathrm{O}\) in \(\mathrm{O}_{2}\)___________ \(\mathrm{Ag}\) in Ag _________________________ \(\mathrm{Cu}\) in \(\mathrm{CuCl}_{2}\)_______

Saccharin $\left(\mathrm{C}_{7} \mathrm{H}_{5} \mathrm{NO}_{3} \mathrm{S}\right)$ is sometimes dispensed in tablet form. Ten tablets with a total mass of 0.5894 g were dissolved in water. The saccharin was oxidized to convert all the sulfur to sulfate ion, which was precipitated by adding an excess of barium chloride solution. The mass of BaSO\(_{4}\) obtained was 0.5032 g. What is the average mass of saccharin per tablet? What is the average mass percent of saccharin in the tablets?

Many oxidation–reduction reactions can be balanced by inspection. Try to balance the following reactions by inspection. In each reaction, identify the substance reduced and the substance oxidized. a. $\mathrm{Al}(s)+\mathrm{HCl}(a q) \rightarrow \mathrm{AlCl}_{3}(a q)+\mathrm{H}_{2}(g)$ b. $\mathrm{CH}_{4}(g)+\mathrm{S}(s) \rightarrow \mathrm{CS}_{2}(l)+\mathrm{H}_{2} \mathrm{S}(g)$ c. $\mathrm{C}_{3} \mathrm{H}_{8}(g)+\mathrm{O}_{2}(g) \rightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(i)$ d. $\mathrm{Cu}(s)+\mathrm{Ag}^{+}(a q) \rightarrow \mathrm{Ag}(s)+\mathrm{Cu}^{2+}(a q)$

Many plants are poisonous because their stems and leaves contain oxalic acid, \(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4},\) or sodium oxalate, \(\mathrm{Na}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\) . When ingested, these substances cause swelling of the respiratory tract and suffocation. A standard analysis for determining the amount of oxalate ion, $\mathrm{C}_{2} \mathrm{O}_{4}^{2-},$ in a sample is to precipitate this species as calcium oxalate, which is insoluble in water. Write the net ionic equation for the reaction between sodium oxalate and calcium chloride, \(\mathrm{CaCl}_{2},\) in aqueous solution.

Using the general solubility rules given in Table 4.1, name three reagents that would form precipitates with each of the following ions in aqueous solution. Write the net ionic equation for each of your suggestions. a. chloride ion \(\quad\) d. sulfate ion b. calcium ion \(\quad\) e. mercury \((1)\) ion, \(\mathrm{Hg}_{2}^{2+}\) c. iron(M) ion \(\quad\) f. silver ion
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