Home / AP Chemistry: 4.2 Net Ionic Reaction – Exam Style questions with Answer- FRQ

AP Chemistry: 4.2 Net Ionic Reaction – Exam Style questions with Answer- FRQ

Question

A student is given the task of determining the I content of tablets that contain KI and an inert, water-soluble sugar as a filler. A tablet is dissolved in 50.0 mL of distilled water, and an excess of 0.20 M\( Pb(NO_3)_2\)(aq) is added to the solution. A yellow precipitate forms, which is then filtered, washed, and dried. The data from the experiment are shown in the table above.

(a) For the chemical reaction that occurs when the precipitate forms, (i) write a balanced, net-ionic equation for the reaction, and

 

                                                                                                                               (ii) explain why the reaction is best represented by a net-ionic equation.

(b) Explain the purpose of drying and weighing the filter paper with the precipitate three times.

(c) In the filtrate solution, is [K] greater than, less than, or equal to Justify \([NO_{3}^{-}]\)? your answer.

(d) Calculate the number of moles of precipitate that is produced in the experiment.

(e) Calculate the mass percent of I in the tablet.

(f) In another trial, the student dissolves a tablet in 55.0 mL of water instead of 50.0 mL of water. Predict whether the experimentally determined mass percent of I will be greater than, less than, or equal to the amount calculated in part

(e). Justify your answer.

g) A student in another lab also wants to determine the I content of a KI tablet but does not have access to Pb\((NO_3)_2\). However, the student does have access to 0.20 M\( AgNO_3\), which reacts with I ̄(aq) to produce AgI(s). The value of Kp for Agl is 8.5 × 10−17.

(i) Will the substitution of \(AgNO_3\) for \(Pb(NO_3)_2\) result in the precipitation of the I- ion from solution? Justify your answer.

(ii) The student only has access to one KI tablet and a balance that can measure to the nearest 0.01 g. Will the student be able to determine the mass of Agl produced to three significant figures? Justify your answer.

▶️Answer/Explanation

a.(i)    \(Pb^{2+} + 2I^{-} → Pbl_{2}\)

a.(ii) The net-ionic equation shows the formation of the\( Pbl_{2}\)(s) from \(Pb^{2+}\)(aq) and \(I^{+}\)(aq) ions, omitting the non-reacting species (spectator ions), \(K^{+}\)(aq) and \(NO_{3} ̄\)(aq).

(b) The filter paper and precipitate must be dried several times (to a constant mass) to ensure that all the water has been driven off.

(c) [\(K^{+}\)] is less than \([NO_{3}\)] because the source of the\( NO_{3}^{-}\), the 0.20 M Pb(NO_{3})_{2}(aq), was added in excess.

(d)1.698 g 1.462 g=0.236 g Pbl2(s)

\(0.236g Pbl_{2}\frac{1molPbl_{2}}{461.0gPbl_{2}}=5.12\times 10^{-4} mol Pbl_{2}\)

(e) \(5.12 × 10^{-4}mol Pbl_{2} ×\frac{2 mol I^{-}}{1 mol Pbl_{2}}\)= 1.02 × 10^{-3} mol I^{-1}\)

    \(1.02 x 10^{3}mol I ̄ ×\frac{126.91 g I^{-}}{1 mol I^{-}}=0.130 g I^{-}\) in one tablet

      \(\frac{0.130 g I^{-}} {0.425 g KI tablet}\)= 0.306 30.6% per KI tablet

(f) The mass percent of\( I^{-}\) will be the same. \(Pb^{2+}\)(aq) was added in excess, ensuring that essentially no I remained in solution. The additional water is removed by filtration and drying, leaving the same mass of dried precipitate.

g (i) Yes. Addition of an excess of 0.20 M \(AgNO_{3}\)(aq) will precipitate all of the I- ion present in the solution because Agl is insoluble, as evidenced by its low value of \(K_{sp}\)

g.(ii) No. If masses can be measured to ±0.01 g, then the mass of the dry Agl(s) precipitate (which is less than 1 g) will be known to only two significant figures.

Question.

\(2NaHCO_{3}(s)\rightarrow Na_{2}CO_{3}+CO_{2}(g)+H_{2}O(g)\)

\( NaHCO_3\)(s) (baking soda) decomposes upon heating to produce \(Na_2CO_3(s) \)and two gaseous products, as shown by the equation above.

(a) A student claims that the reaction is an oxidation-reduction reaction because the oxidation number of carbon changes. Do you agree with the claim? In your answer include the oxidation number of carbon in each of the three carbon-containing species in the reaction. The student conducts an experiment to determine the composition of a mixture of \(NaHCO_3\) (molar mass 84.01 g/mol) and \(Na_2CO_3\) (molar mass 105.99 g/mol). The student places a sample of the mixture into a preweighed test tube that is attached to a container that holds a drying agent. The student heats the test tube strongly with a Bunsen burner for 10 minutes, during which time all of the water produced by the reaction is captured by the drying agent. The following table shows the data the student recorded during the experiment.

(b) Calculate the number of moles of\( NaHCO_3(s)\) present in the mixture in the test tube before the reaction was initiated.
(c) Determine the mass percent of\( NaHCO_3(s)\) in the mixture.
(d) If the student spills some of the mixture out of the test tube after weighing the test tube and mixture and before heating, how would this error affect the mass percent of \(NaHCO_3\) calculated in part (c) ? Justify your answer. When a sample of pure\( Na_2CO_3 \)is placed in distilled water, the student observes that the pH of the solution increases significantly. This process is represented by the balanced net-ionic equation shown below.

                                    \(CO_{3}^{2-}(aq)+H_2O{l}\rightleftharpoons HCO_{3}^-+OH^{-}(aq)\)

(e) The student prepares a 0.10 M \(Na_2CO_3(aq)\) solution and measures the pH of the solution to be 11.65.
(i) Calculate\( [OH^{-}]\) in the \(Na_2CO_3\)(aq) solution.
(ii) Write the expression for \(K_b\) for the carbonate ion.
(iii) Calculate the value of \(K_b \)for the carbonate ion. The student adds some 1.0 M Sr\((NO_3)_2\)(aq) to the 0.10 M\( Na_2CO_3(aq)\) and observes the formation of a precipitate.
(f) Write the balanced net-ionic equation for the reaction between Sr\((NO_3)_2\) and \(Na_2CO_3\) that produces the precipitate.

▶️Answer/Explanation

(a) No. The oxidation number of carbon is +4 in each of the three carbon-containing species.

(b)     

       

(c) \(0.0188mol NaHCO_{3}\times \frac{84.01g NaHCO_{3}}{1molNaHCO_{3}}\frac{1.58g}{(17.648g-15.825g)}\times =86.7%\)

(d) The calculated mass percent would be smaller than the actual value. Less water would be collected, so there would appear to be less\( NaHCO_3\) in the sample.

(e)(i) \(pOH = 14.00 – 11.65 = 2.35\)
\([OH^−] = 10-2.35 = 4.5\times 10^-{3}\)

e(ii)  \(k_b=\frac{[HCO_{3}^{-}][OH^-]}{CO_{3}^{2-}}\)

e(iii)  \(K_b=\frac{(4.5\times 10^{-3})\times (4.5\times 10^{-3})}{0.10-(4.5\times 10^{-3})}\approx \frac{(4.5\times 10^{-3})^2}{0.10}= 2.0\times 10^{-4}\)

(f) \(Sr^{2+}CO_{3}^{2-}\rightarrow SrCO_{3}\)

Question

 The addition of 0.100M \(AgNO_3\) (aq) to a beaker containing 0.100 M NaCl (aq) results in the
formation of a precipitate.
a. What is the identity of the precipitate?
b. Write the net ionic equation showing this precipitate’s formation.
c. A concentrated solution of NH3 (aq) was added to the beaker containing the precipitate. As a result, the precipitate dissolved. Write equations showing the chemical reaction which takes place when the ammonia solution is added to the beaker.

▶️Answer/Explanation

Answer:

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