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Chapter 4: Problem 53

Calculate the mass of \(\mathrm{KI}\) in grams required to prepare \(5.00 \times 10^{2} \mathrm{~mL}\) of a \(2.80 \mathrm{M}\) solution.

Short Answer

Expert verified
The mass of KI required to prepare the solution is 232.4 grams.

Step by step solution

01

Convert Volume to Liters

The volume is given in milliliters. We need to convert this to liters, since the volume in the formula for molarity is in liters. Recall that 1 Liter is equivalent to 1000 milliliters. Therefore, \(500 mL = 0.500 L\).
02

Calculate the Number of Moles Needed

Using the formula \(M = \frac {n}{V}\), we can determine the number of moles of KI required. Given the molarity of the solution is 2.80 M and we've already converted the volume to 0.500 L, we rearrange the formula \(n = M \times V\) to get \(n= 2.80 \times 0.500 = 1.4 moles\). Therefore, we need 1.4 moles of KI to prepare the solution.
03

Convert Moles to Grams

We have found that the number of moles of KI needed is 1.4 moles. Now we use the molar mass of KI to convert this to grams. Recall that the molar mass of KI is about 166 g/mol. Therefore, the mass of KI required can be calculated as \(mass = n \times molar~mass = 1.4 \times 166 = 232.4 grams\).

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Most popular questions from this chapter

Give oxidation numbers for the underlined atoms in the following molecules and ions: (a) \(\underline{\mathrm{Cs}_{2} \mathrm{O}},\) (b) \(\mathrm{Ca} \underline{\mathrm{I}}_{2}\), (c) \(\underline{\mathrm{Al}_{2} \mathrm{O}_{3}}\) (d) \(\mathrm{H}_{3} \mathrm{As} \mathrm{O}_{3},\) (e) \(\underline{\mathrm{Ti} \mathrm{O}_{2}},\) (f) \(\underline{\mathrm{Mo}} \mathrm{O}_{4}^{2-}\), (g) \(\underline{\mathrm{Pt} \mathrm{Cl}_{4}^{2-}}\) (h) \(\underline{\mathrm{Pt}} \mathrm{Cl}_{6}^{2-}\) (i) \(\underline{\operatorname{Sn} F}_{2}\) (j) \(\underline{\mathrm{ClF}_{3},}\) (k) \(\underline{\mathrm{Sb}} \mathrm{F}_{6}^{-}\)

Classify these reactions according to the types discussed in the chapter: (a) \(\mathrm{Cl}_{2}+2 \mathrm{OH}^{-} \longrightarrow \mathrm{Cl}^{-}+\mathrm{ClO}^{-}+\mathrm{H}_{2} \mathrm{O}\) (b) \(\mathrm{Ca}^{2+}+\mathrm{CO}_{3}^{2-} \longrightarrow \mathrm{CaCO}_{3}\) (c) \(\mathrm{NH}_{3}+\mathrm{H}^{+} \longrightarrow \mathrm{NH}_{4}^{+}\) (d) \(2 \mathrm{CCl}_{4}+\mathrm{CrO}_{4}^{2-} \longrightarrow\) \(2 \mathrm{COCl}_{2}+\mathrm{CrO}_{2} \mathrm{Cl}_{2}+2 \mathrm{Cl}^{-}\) (e) \(\mathrm{Ca}+\mathrm{F}_{2} \longrightarrow \mathrm{CaF}_{2}\) (f) \(2 \mathrm{Li}+\mathrm{H}_{2} \longrightarrow 2 \mathrm{LiH}\) (g) \(\mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}+\mathrm{Na}_{2} \mathrm{SO}_{4} \longrightarrow 2 \mathrm{NaNO}_{3}+\mathrm{BaSO}_{4}\) (h) \(\mathrm{CuO}+\mathrm{H}_{2} \longrightarrow \mathrm{Cu}+\mathrm{H}_{2} \mathrm{O}\) (i) \(\mathrm{Zn}+2 \mathrm{HCl} \longrightarrow \mathrm{ZnCl}_{2}+\mathrm{H}_{2}\) (j) \(2 \mathrm{FeCl}_{2}+\mathrm{Cl}_{2} \longrightarrow 2 \mathrm{FeCl}_{3}\)

A \(5.00 \times 10^{2}-\mathrm{mL}\) sample of \(2.00 \mathrm{M} \mathrm{HCl}\) solution is treated with \(4.47 \mathrm{~g}\) of magnesium. Calculate the concentration of the acid solution after all the metal has reacted. Assume that the volume remains unchanged.

Based on oxidation number, explain why carbon monoxide (CO) is flammable but carbon dioxide \(\left(\mathrm{CO}_{2}\right)\) is not.

Describe the basic steps involved in gravimetric analysis. How does this procedure help us determine the identity of a compound or the purity of a compound if its formula is known?
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