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Chapter 4: Problem 76

A \(30.0-\mathrm{mL}\) sample of an unknown strong base is neutralized after the addition of \(12.0 \mathrm{~mL}\) of a \(0.150 \mathrm{M} \mathrm{HNO}_{3}\) solution. If the unknown base concentration is \(0.0300 M\), give some possible identities for the unknown base.

Short Answer

Expert verified
Possible identities for the unknown strong base are Sodium hydroxide (NaOH), Potassium hydroxide (KOH), Calcium hydroxide (Ca(OH)₂), and Barium hydroxide (Ba(OH)₂). These bases can neutralize with HNO₃, and they have the same moles (0.00180 mol) and concentration (0.0300 M) as given in the problem.

Step by step solution

01

Calculate the moles of the strong acid HNO₃

To calculate the moles of the acid, we can use the formula moles = molarity x volume. In this case, the molarity of HNO₃ is given as 0.150 M, and the volume is given as 12.0 mL. Moles of HNO₃ = (0.150 mol/L) x (12.0 mL x 10⁻³ L/mL) = 0.00180 mol
02

Calculate the moles of the unknown base

Since the moles of acid = moles of base in a neutralization reaction, we have: Moles of unknown base = moles of HNO₃ = 0.00180 mol
03

Calculate the volume of the unknown base

We are given the concentration of the unknown base as 0.0300 M and now we know the moles of the base as 0.00180 mol, we can calculate the volume of the unknown base using the formula volume = moles/concentration. Volume of unknown base = 0.00180 mol / 0.0300 mol/L = 0.0600 L
04

Identify possible strong bases

We can now identify some strong bases based on their possible reactions with HNO₃. Some common strong bases are: 1. Sodium hydroxide (NaOH) 2. Potassium hydroxide (KOH) 3. Calcium hydroxide (Ca(OH)₂) 4. Barium hydroxide (Ba(OH)₂) These are just a few examples of possible strong bases. More options could be present, as long as they neutralize with HNO₃ and have the same moles and concentration as given in the problem.

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Most popular questions from this chapter

Which of the following solutions of strong electrolytes contains the largest number of ions: \(100.0 \mathrm{~mL}\) of \(0.100 \mathrm{M} \mathrm{NaOH}\), \(50.0 \mathrm{~mL}\) of \(0.200 \mathrm{M} \mathrm{BaCl}_{2}\), or \(75.0 \mathrm{~mL}\) of \(0.150 \mathrm{M} \mathrm{Na}_{3} \mathrm{PO}_{4}\) ?

A \(230 .-\mathrm{mL}\) sample of a \(0.275-M \mathrm{CaCl}_{2}\) solution is left on a hot plate overnight; the following morning, the solution is \(1.10 M\). What volume of water evaporated from the \(0.275 \mathrm{M} \mathrm{CaCl}_{2}\) solution?

Balance each of the following oxidation-reduction reactions by using the oxidation states method. a. \(\mathrm{C}_{2} \mathrm{H}_{6}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightarrow \mathrm{CO}_{2}(\mathrm{~g})+\mathrm{H}_{2} \mathrm{O}(g)\) b. \(\mathrm{Mg}(s)+\mathrm{HCl}(a q) \rightarrow \mathrm{Mg}^{2+}(a q)+\mathrm{Cl}^{-}(a q)+\mathrm{H}_{2}(g)\) c. \(\mathrm{Co}^{3+}(a q)+\mathrm{Ni}(s) \rightarrow \mathrm{Co}^{2+}(a q)+\mathrm{Ni}^{2+}(a q)\) d. \(\mathrm{Zn}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \rightarrow \mathrm{ZnSO}_{4}(a q)+\mathrm{H}_{2}(g)\)

A mixture contains only \(\mathrm{NaCl}\) and \(\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3} .\) A \(0.456-\mathrm{g}\) sample of the mixture is dissolved in water, and an excess of \(\mathrm{NaOH}\) is added, producing a precipitate of \(\mathrm{Fe}(\mathrm{OH})_{3} .\) The precipitate is filtered, dried, and weighed. Its mass is \(0.107\) g. Calculate the following. a. the mass of iron in the sample b. the mass of \(\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}\) in the sample c. the mass percent of \(\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}\) in the sample

What acid and what base would react in aqueous solution so that the following salts appear as products in the formula equation? Write the balanced formula equation for each reaction. a. potassium perchlorate b. cesium nitrate c. calcium iodide
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