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Chapter 14: Problem 61

How would you prepare \(1600 \mathrm{~mL}\) of a \(\mathrm{pH}=1.50\) solution using concentrated \((12 M) \mathrm{HCl} ?\)

Short Answer

Expert verified
To prepare $1600 \mathrm{~mL}$ of a $\mathrm{pH} = 1.50$ solution using concentrated $(12 M) \mathrm{HCl}$, first calculate the molarity of the resulting solution using the pH equation, which gives $[H^+] = 0.0316M$. Next, determine the volume of concentrated HCl required using the dilution equation, which gives $V1 = 4.21 \mathrm{~mL}$. Finally, prepare the solution by measuring 4.21 mL of concentrated $12 M \mathrm{HCl}$, carefully adding it to $1600 \mathrm{~mL}$ of distilled water, and mixing gently until homogeneous.

Step by step solution

01

Calculate the molarity of the resulting solution

To find the molarity of the resulting solution, we use the pH equation: \( pH = -\log_{10} [H^+] \) Rearrange the equation to find [H+]: \( [H^+] = 10^{-pH} \) Plug in the given pH value: \[ [H^+] = 10^{-1.50} \] Calculate the molarity: \[ [H^+] =0.0316M \]
02

Determine the volume of concentrated HCl required

To find the volume of concentrated HCl needed, we use the dilution equation (M1V1 = M2V2): M1 = Concentration of the stock solution (12 M) V1 = ? (this is the volume of stock solution we need to determine) M2 = concentration of the diluted solution (0.0316 M) V2 = volume of the diluted solution (1600 mL) Plugging the numbers into the equation M1V1 = M2V2: \( 12V1 = 0.0316 \times 1600 \) Solve for V1: \( V1 = \frac{0.0316 \times 1600}{12} \) Calculate the volume, V1: \( V1 = 4.21 \mathrm{~mL} \)
03

Prepare the 1600 mL pH 1.50 solution

To prepare the solution, follow these steps: 1. Measure 4.21 mL of the concentrated 12 M HCl using a graduated cylinder or a pipette. 2. Pour the 4.21 mL of HCl into a 1600 mL volumetric flask. 3. Fill the volumetric flask with distilled water about ¾ of the way and gentle mix the solution. 4. Add more distilled water until the solution reaches the 1600 mL mark on the volumetric flask. 5. Mix the solution gently until homogeneous. Now, you have prepared 1600 mL of a pH 1.50 solution using concentrated 12 M HCl.

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Most popular questions from this chapter

Consider \(50.0 \mathrm{~mL}\) of a solution of weak acid \(\mathrm{HA}\left(K_{\mathrm{a}}=\right.\) \(1.00 \times 10^{-6}\) ), which has a pH of \(4.000\). What volume of water must be added to make the \(\mathrm{pH}=5.000 ?\)

What are the major species present in the following mixtures of bases? a. \(0.050 \mathrm{M} \mathrm{NaOH}\) and \(0.050 \mathrm{M} \mathrm{LiOH}\) b. \(0.0010 \mathrm{M} \mathrm{Ca}(\mathrm{OH})_{2}\) and \(0.020 \mathrm{M} \mathrm{RbOH}\) What is \(\left[\mathrm{OH}^{-}\right]\) and the \(\mathrm{pH}\) of each of these solutions?

Calculate the \(\mathrm{pH}\) of a \(0.200-M\) solution of \(\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{NHF}\). Hint: \(\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{NHF}\) is a salt composed of \(\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{NH}^{+}\) and \(\mathrm{F}^{-}\) ions. The principal equilibrium in this solution is the best acid reacting with the best base; the reaction for the principal equilibrium is \(\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{NH}^{+}(a q)+\mathrm{F}^{-}(a q) \rightleftharpoons\) \(\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{~N}(a q)+\mathrm{HF}(a q) \quad K=8.2 \times 10^{-3}\)

Which of the following represent conjugate acid-base pairs? For those pairs that are not conjugates, write the correct conjugate acid or base for each species in the pair. a. \(\mathrm{H}_{2} \mathrm{O}, \mathrm{OH}^{-}\) c. \(\mathrm{H}_{3} \mathrm{PO}_{4}, \mathrm{H}_{2} \mathrm{PO}_{4}^{-}\) b. \(\mathrm{H}_{2} \mathrm{SO}_{4}, \mathrm{SO}_{4}^{2-}\) d. \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}, \mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}^{-}\)

The \(\mathrm{pH}\) of a \(0.016-M\) aqueous solution of \(p\) -toluidine \(\left(\mathrm{CH}_{3} \mathrm{C}_{6} \mathrm{H}_{4} \mathrm{NH}_{2}\right)\) is 8.60. Calculate \(K_{\mathrm{b}}\).
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