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- A solution contains both NaHCO3 and Na2CO3. Titration of a 50.00 mL portion to a phenolphthalein end point requires 21.25 mL of 0.1385 M HCl. A second 50.00 mL aliquot requires 45.48 mL of the HCl solution when titrated to a bromocresol green end point. Calculate the molar concentration of Na2CO3 in the original solution. (Do not include the unit for molarity. Enter your answer to three significant figures.)Excess Cu(OH)2 is placed in a beaker and nitric acid is added to dissolve some of the copper oxide. Asa strong acid, nitric acid is fully dissociated. Write the relevant reactions for processes in the beaker. The complete dissociation of HNO3 is aRXN0, as shown. Two reactions RXN1 and RXN2 are needed to capture the chemistry in the beaker.RXN0: HNO3 + H2O -->H3O+ + NO3-Under what circumstances, if any, does a sample of solid AgCl completely dissolve in pure water?
- Zhongli is a speleologist tasked to analyze the CaCO₃ content of a limestone stalactite. A 5.0000-g sample was dissolved in 25.00 mL of 1.350 M HCl, it was then heated to expel any CO₂ formed. The excess HCl was titrated to a phenolphthalein end point, it used 37.50 mL of 0.1200 M NaOH. What is the reaction for the digestion of the limestone sample A. 2 NaOH + CaCO₃ ⇌ Na₂CO₃ + Ca(OH)₂ B. CaCO₃ ⇌ CaO + CO₂ C. 2 HCl + CaCO₃ ⇌ CaCl₂ + H₂O + CO₂ D. NaOH + HCl ⇌ NaCl + H₂OWhich compound, FeCO3 or PbBr2, is more soluble in acid than in base? Why?A student dissolved a compound in water and added hydrochloric acid. No precipitate formed. Next, she bubbled H2S into this solution, but again, no precipitate formed. However, when she made the solution basic with ammonia and bubbled in H2S , a precipitate formed. Which of the following are possible as the cation in the compound? - CA2+ - Ag+ - Cd2+ - Mn2+
- 1. If the potassium hydrogen phthalate is not completely dry, how would it affect the reported molar concentration (molarity) of the NaOH solution in Part A? Explain. 2. In Part A, the mass of KHC;H4O4 is measured to the nearest 0.0001 g. However, the volume of water used to dissolve the KHP does not need to be precise. Explain why the amount of water added to KHP has no effect on the experimental results. 3. Identify two possible sources of experimental error in this experiment, and describe the effect of each error in the determination of the molar concentration (molarity) of the acid solution in Part B.Consider the titration of the weak acid, benzoic acid, HC7H5O2. Its acid dissociation reaction is: HC7H5O2 (aq) + H2O (l) ↔ C7H5O2- (aq) + H3O+ (aq) A 25.00 mL sample of a solution of benzoic acid, concentration unknown, is titrated with 0.0500M NaOH solution. A plot of the titration is shown below. 1. what is the pKa (approximately) of benzoic acid? Its Ka? 2. on the plot, indicate the buffering region of the titration 3. From the pH at the equivalence point, estimate the pKb of benzoate ion (conjugate base to benzoic acid)______________[Remember, at the equivalence point, C7H5O2- (aq) + H2O (l) ↔ HC7H5O2 (aq) + OH- (aq) ]What will be the appropriate pH of a buffer prepared by mixing 100 ml of 0.1 M Na2HPO4 and 100 ml of 0.1 M NaH2PO4? (For H3PO4, pKa1 = 2.1; pKa2 = 6.8; pKa3 = 12.5) Ans in 2 significant figures
- 23. lodide ion (1) is the conjugate base of hydroiodic acid (HI). Why doesn't sodium iodide cause an appreciable increase in the pH of water when it dissolves into Na* and I ions? (a) The Na' is acidic and neutralizes the basicity of I (b) It is a stronger acid than it is a base in water, so Nal actually lowers the pH when dissolved. (c) There are no H₂O* ions present in the solution that could react with I. (d) At least a small amount of HI must be present in order for I to act as a base to raise the pH. (e) HI is a strong acid that reacts completely, which makes I a correspondingly weak base. 24. K, for methylamine (CH3NH₂) is the equilibrium constant for which reaction? (a) CHÍNH, + HO - CHÍNH + HO CH₂NH3 + OH* = CHÍNH + H2O CH₂NH™ + H₂O (b) CH₂NH₂ + H₂O (C) CHÍNH, + HO (d) CH₂NH₂ + OH (e) None of the aboveA 0.6000 g sample contains NaHCO₃, Na₂CO₃ ,and NaOH, either alone or in permissiblecombination. Titration of a 50.0-mL portion toa phenolphthalein end point requires 24.27mL of 0.100 M HCl. A second 50.0-mL aliquotrequires 51.11 mL of the HCl when titrated toa bromocresol green end point. Deduce thecomposition, and calculate the percentcomposition of the substances in the sample.When 10 drops of 0.1 M Co2+ is acidified using 20 drops 6.0 M CH3COOH and a pinch of solid NaNO2 is added then placed in a warm water bath, an orange solution is observed. Write the net ionic equation associated with the formation of the orange solution and indentify which species is responsible for this color change.