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Chapter 4: Problem 61

(a) Calculate the molarity of a solution that contains 0.175 mol \(\mathrm{ZnCl}_{2}\) in exactly \(150 \mathrm{~mL}\) of solution. (b) How many moles of protons are present in \(35.0 \mathrm{~mL}\) of a \(4.50 \mathrm{M}\) solution of nitric acid? (c) How many milliliters of a $6.00 \mathrm{M} \mathrm{NaOH}\( solution are needed to provide 0.350 mol of \)\mathrm{NaOH} ?$

Short Answer

Expert verified
(a) The molarity of the ZnCl₂ solution is 1.17 M. (b) There are 0.1575 moles of protons present in 35.0 mL of a 4.50 M solution of nitric acid. (c) To provide 0.350 mol of NaOH, 58.3 mL of a 6.00 M NaOH solution is needed.

Step by step solution

01

Identify the given values

We are given the number of moles of ZnCl₂ (0.175 mol) and the volume of the solution (150 mL). We need to calculate the molarity of the solution.
02

Convert the volume to liters

Since molarity requires the volume to be in liters, we need to convert 150 mL to liters. Recall that 1 L = 1000 mL. Therefore, the volume in liters is: \(V (L) = \frac{150}{1000} = 0.15 L\)
03

Calculate the molarity

Now, use the formula M = n/V to calculate the molarity of the solution: \(M = \frac{n}{V} = \frac{0.175 \text{ mol}}{0.15 \text{ L}} = 1.17 \text{ M}\) Part (b)
04

Identify the given values

We are given the volume of nitric acid solution (35.0 mL) and its molarity (4.50 M). We need to find the number of moles of protons present in the solution.
05

Convert the volume to liters

Convert the volume of the nitric acid solution from milliliters to liters: \(V (L) = \frac{35.0}{1000} = 0.035 L\)
06

Find the number of moles of protons

Now, we can use the formula M = n/V to find the number of moles of protons in the solution: \(n = M \times V = 4.50 \text{ M} \times 0.035 \text{ L} = 0.1575 \text{ mol}\) There are 0.1575 moles of protons present in 35.0 mL of a 4.50 M solution of nitric acid. Part (c)
07

Identify the given values

We are given the molarity of the NaOH solution (6.00 M) and the number of moles of NaOH (0.350 mol). We need to find the volume of the NaOH solution in milliliters.
08

Calculate the volume in liters

Use the formula M = n/V to find the volume of the NaOH solution in liters: \(V (L) = \frac{n}{M} = \frac{0.350 \text{ mol}}{6.00 \text{ M}} = 0.0583 \text{ L}\)
09

Convert the volume to milliliters

Now, convert the volume of the NaOH solution from liters to milliliters: \(V (mL) = 0.0583 \text{ L} \times 1000 = 58.3 \text{ mL}\) To provide 0.350 mol of NaOH, 58.3 mL of a 6.00 M NaOH solution is needed.

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Most popular questions from this chapter

Using the activity series (Table 4.5 ), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (a) Nickel metal is added to a solution of copper(II) nitrate, (b) a solution of zinc nitrate is added to a solution of magnesium sulfate, (c) hydrochloric acid is added to gold metal, (d) chromium metal is immersed in an aqueous solution of cobalt(II) chloride, (e) hydrogen gas is bubbled

When carbon dioxide dissolves in water, it is in equilibrium with carbonic acid \(\mathrm{H}_{2} \mathrm{CO}_{3},\) which is a weak electrolyte. What solutes are present in aqueous solution of this compound? Write the chemical equation for the ionization of \(\mathrm{H}_{2} \mathrm{CO}_{3}\)

Write balanced net ionic equations for the reactions that occur in each of the following cases. Identify the spectator ion or ions in each reaction. (a) \(\mathrm{Ba}(\mathrm{OH})_{2}(a q)+\mathrm{FeCl}_{3}(a q) \longrightarrow\) (b) $\mathrm{ZnCl}_{2}(a q)+\mathrm{Cs}_{2} \mathrm{CO}_{3}(a q) \longrightarrow$ (c) $\mathrm{Na}_{2} \mathrm{~S}(a q)+\operatorname{CoSO}_{4}(a q) \longrightarrow$

Ignoring protolysis reactions (i.e. proton transfer reaction), specify what ions are present in a solution upon dissolving each of the following substances in water: (a) \(\mathrm{Li}_{2} \mathrm{CO}_{3},\) (b) \((\mathrm{NH} 4)_{3} \mathrm{PO}_{4}\) (d) \(\mathrm{NaPF}_{6^{\circ}}\) (c) \(\mathrm{Na}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\)

State whether each of the following statements is true or false. Justify your answer in each case. (a) \(\mathrm{NH}_{3}\) contains no \(\mathrm{OH}^{-}\) ions, and yet its aqueous solutions are basic. (b) HF is a strong acid. (c) Although sulfuric acid is a strong electrolyte, an aqueous solution of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) contains more \(\mathrm{HSO}_{4}^{-}\) ions than \(\mathrm{SO}_{4}^{2-}\) ions.
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