Concept explainers
Balance these equations for reactions in acidic solution.
a.
b.
c.
d.
e.
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EBK GENERAL CHEMISTRY
- Three acid samples are prepared for titration by 0.01 M NaOH: 1 Sample 1 is prepared by dissolving 0.01 mol of HCl in 50 mL of water. 2 Sample 2 is prepared by dissolving 0.01 mol of HCl in 60 mL of water. 3 Sample 3 is prepared by dissolving 0.01 mol of HCl in 70 mL of water. a Without performing a formal calculation, compare the concentrations of the three acid samples (rank them from highest to lowest). b When the titration is performed, which sample, if any, will require the largest volume of the 0.01 M NaOH for neutralization?arrow_forwardClassify the following as acid-base reactions or oxidation-reduction reactions: (a) Na2S(aq)+2HCl(aq)2NaCl(aq)+H2(g) (b) 2Na(s)+2HCl(aq)2NaCl(aq)+H2(g) (c) Mg(s)+Cl2(g)MgCl2(s) (d) MgO(s)+2HCl(aq)MgCl2(aq)+H2+O(l) (e) K3P(s)+2O2(g)K3PO4(s) (f) 2KOH(aq)+H3PO4(aq)K3PO4(aq)+3H2O(l)arrow_forwardComplete the right side of each of the following molecular equations. Then write the net ionic equations. Assume all salts formed are soluble. Acid salts are possible. a Ca(OH)2(aq) + 2H2SO4(aq) b 2H3PO4(aq) + Ca(OH)2(aq) c NaOH(aq) + H2SO4(aq) d Sr(OH)2(aq) + 2H2CO3(aq)arrow_forward
- Consider four beakers. Beaker A has an aqueous solution of NaOH in which the OH- ions are represented by blue circles. Beaker B has a weak acid; HX is represented by red circles. Beaker C has a weak acid; H2X is represented by green circles. Beaker D has a weak acid; H3X is represented by yellow circles. X- ions are represented by triangles. Match the pictorial representations with the reactions given below. (a) HX(aq)+OH(aq) X(aq)+H2O(b) H2X(aq)+2OH(aq) X(aq)+2H2O(c) H3X(aq)+3OH(aq) X(aq)+3H2Oarrow_forwardWhen the following solutions are mixed together, what precipitate (if any) will form? a. FeSO4(aq) + KCl(aq) b. Al(NO3)3(aq) + Ba(OH)2(aq) c. CaCl2(aq) + Na2SO4(aq) d. K2S(aq) + Ni(NO3)2(aq)arrow_forwardDraw the flow diagram for a calculation that illustrates how to use a titration to determine the concentration of a solution of HNO3, by reaction with 1.00 g Na2CO3.arrow_forward
- A 0.500-L sample of H2SO4 solution was analyzed by taking a 100.0-mL aliquot and adding 50.0 mL of 0.213 M NaOH. After the reaction occurred, an excess of OH ions remained in the solution. The excess base required 13.21 mL of 0.103 M HCl for neutralization. Calculate the molarity of the original sample of H2SO4. Sulfuric acid has two acidic hydrogens.arrow_forwardYou are given four different aqueous solutions and told that they each contain NaOH, Na2CO3, NaHCO3, or a mixture of these solutes. You do some experiments and gather these data about the samples. Sample A: Phenolphthalein is colorless in the solution. Sample B: The sample was titrated with HCl until the pink color of phenolphthalein disappeared, then methyl orange was added. The solution became pink. Methyl orange changes color from pH 3.01 (red) to pH 4.4 (orange). Sample C: Equal volumes of the sample were titrated with standardized acid. Using phenolphthalein as an indicator required 15.26 mL of standardized acid to change the phenolphthalein color. The other sample required 17.90 mL for a color change using methyl orange as the indicator. Sample D: Two equal volumes of the sample were titrated with standardized HCl. Using phenolphthalein as the indicator, it took 15.00 mL of acid to reach the equivalence point; using methyl orange as the indicator required 30.00 mL HCl to achieve neutralization. Identify the solute in each of the solutions.arrow_forwardMalonic acid, H2C3H2O4 (aq), is a diprotic acid, so 2 moles of hydroxide ions are required per mole of malonic acid for complete neutralization. A.) Write the balanced chemical equation for the reaction of malonic acid with potassium hydroxide. B.) Calculate the molar concentration of the malonic acid if 38.17 mL of 0.315 M potassium hydroxide was required to neutralize 25.0 mL of malonic acid to a phenolphthalein end point. C.) Calculate the mass percent concentration of malonic acid using the molar concentration calculated in part b and assuming the density of the solution is 1.01 g/mL.arrow_forward
- Balance each ACIDIC net ionic equation below. Be sure to include water and hydrogen ions, as required, in the final balanced, net ionic equation. Mno, 1) _Mo24037 + → _Moog _Mn2 Ag + NO, → _Ag*1 NO Mno," _c,0,2 3) → _Mit2 _Co2 _NO, - _Mno, 5) → _NO, Mn*2 . _Cr,0 +1 → 6) Mno, 7) > _Mn*2 P + _NO, - 8) > NO + 9) C+3 10) Seq? + _CI > Seo 2)arrow_forwardA)When working in the lab, you are measuring the pH of a system. The pH meter reads 4.34. What is the concentration of [H3O+] in solution? B)You have created a solution of NaOH by dissolving NaOH in water. You determine that the [OH-] concentration in solution is 4.37 x 10-9. What is the pOH of the solution? C)What is the pH of a solution containing an [H3O+] = 9.67 x 10-3?arrow_forwardSpecialized cells in the stomach release HCl in order to aid in digestion. If these cells release too much HCl, the excess acid can be neutralized with antacids such as TUMS which contain calcium carbonate in order to avoid discomfort. In order to test commercial antacids, a chemist uses 0.160 M HCl to stimulate the acid concentration in the stomach. First, provide a correctly balanced reaction equation for the reaction between hydrochloric acid and calcium carbonate (note that this reaction produces H2O(l) and CO2(g)). Then show how to determine and calculate the amount of stimulated stomach acid (in mL) that would react completely with one extra strength TUMS tablet which contains 7.50x10^2 mg of calcium carbonate. you must use the factor-label(conversion-factor) method for all conversions. Use significant figures and include units where applicable.arrow_forward
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