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Q: prove that for the weak acid CH3COOH and its conjugate base CH3COO- then (Ka x Kp = Kw ).
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- Exercise 3. ldentify all the Bronsted acids and bases in the following equations: (a) NH3 + HCI NH,* + CH (b) HSO; + CN- HCN + SO,- (c) H,PO, + CO;- HPO,2- + HCO;Exercise Find fand cind for (a) an aqueous solution of HCN and KCN; (b) an aqueous solution of HCN and KCl; (c) an aqueous solution of the weak diprotic acid H₂SO3. [Answers: (a) 4, 3; (b) 4, 3; (c) 3, 2.]EXERCISE II -11 1. A chemist,, Hishes to prepare 100.0 mL of a buffer of pH 10.0000 using the base methyl amine, CH,NH2, ánd its salt, CH;NH2, and its salt, CH3NH;CI. (a) What should be the ratio of base to salt to obtain a pH of 10.00? (b) If he makes the solution 0.05000 M CH3NH2, how many moles of methyl ammonium chloride should he add to get the desired pH ? Kp = 5.00 x 104 2. A buffer solution is prepared by dissolving 4.7 g of nitrous acid, HNO2 , and 13.8 g of sodium nitrite, NaNO2, in 1.0 liter of solution. (a) Calculate the pH of the buffer. (b) Calculate the pH of the solution which results when the following are added to separate 100 mL portions of the buffer: (i) 5.0 mmol of HCI; (ii) 5.0 mmol of NaOH. Ka = 4.5 x 104 %3D 3. What change in pH will occur when 0.050 mmol of HOAC (Ka= 1.78 x 10) is added to 100.0 mL of a buffer solution that is 0.1000 M HOAC and 0.1000 M NAOAC? Assume no change in volume.
- pH practice a.) determine the pH of a nitric acid solution (HNO3) that has been prepared by mixing 2.0 mL of 1.0 M HNO3 with 98.0 mL of water b.) determine the pH of a 25 mL carbonic acid solution (H2CO3) with a concentration of 5.7 x 10-5 M. assume all the protons will dissociate from the acid and react with water to form hydronium ions. c.) determine the pH and pOH of a NaOH solution that has been prepared by diluting 20.0 mL of 6.0 M NaOH with 80.0 mL of water. d.) determine the pH and pOH of a Ca(OH)2 solution that has been prepared by mixing 0.26 g of Ca(OH)2 pellets in 750 mL of water.Exercise 6b. Arrange the solutions in order of increasing acidity: NaCl, NH4CI, KCN, NaOH, NaCH3COO, NaC3H5O3, Nicotine, C2H5NH3Cl HA and HB are both weak acids in water, and HA is a stronger acid than HB. Which of the following statements is correct? A) A is a stronger base than B, which is a stronger base than H₂O, which is a stronger base than Cl-. B) B is a stronger base than A, which is a stronger base than H₂O, which is a stronger base than Cl-. C) B is a stronger base than A, which is a stronger base than Cl, which is a stronger base than H₂O. D) CI is a stronger base than A, which is a stronger base than B, which is a stronger base than H₂O. E) None of these (A-D) is correct.Exercise 1: Calculate the pH of the acidic solution obtained by mixing 100 mL of (pH=2) of HC1 with 400 mL of (pH= 3) of HNO3.
- Review I Constants I Periodic Table I J I MII V Calculate the [H3O*] for each of the following measurements of pH. [H3O Ox10-4 M Submit Previous Answer Correct A pH less thar 10-7. s considered acidic, and the hydronium ion concentration h; " be greater than [H3 O+] = 10-pH – 10-3.4 = 4.0 x 10-4 M Part D beer, pH 4.6 Express your answer to two significant figures and include the appropriate units. HẢ [H,O*] = Value Units Submit Request AnswerPractice Exercise 1If you complete and balance the following oxidation–reduction reaction in basic solutionNO2-(aq)+ Al(s)---->NH3(aq) + Al(OH)4-(aq) how many hydroxide ions are there in the balanced equation(for the reaction balanced with the smallest whole-numbercoefficients)?(a) One on the reactant side (b) One on the product side(c) Four on the reactant side (d) Seven on the product side(e) NoneEXERCISE II- 2 1. A 2.00 -mL sample of a 0.100 M solution of KMNO, is mixed with 3.00 mL of a 0.800 M solution of KMNO4 . Calculate the molarity of the final solution, assuming that the volumes are additive. 2. 40.0 mL of a 0.150 M HCI solution is mixed with 60.0 mL of 0.200 M NaOH. Is the resulting solution acidic, basic, or neutral? Calculate the molarity of the reactant which is in excess. 3. (a) If 10.0 mL of H2SO4 (sp. Gr. 1.50, containing 48.7% of combined SO3 by weight) is diluted to 400 mL, what is the normality of the solution as an acid? (b) What volume of 6.00 M H2SO4 should be added to this in order to make the resulting mixture 1.00N as an acid? FW's : H2SC4 = 98; SO3 = 80 %3D %3D 4. A 500-mL graduated flask contains 150 mL of 0.200 N H2SO4. By adding a more concentrated H,SO4, the solution is brought up to mark and after mixing is found to be 0.300 N. What was the normality of the acid that was added? 5. At 25°C, what changes in pH occur when (a) 0.0250 M HCI (b) 0.0250 M…
- Exercise 4: 53 g of NazCO; are dissolved in 1 dm' of de-ionised water. Caleulate (a) molar mass of NazCO: (b) number of moles of Na2CO3 in 53 g (c) the concentration of the solution in mol dm.Consider the following beakers. Each contains a solution of the hypothetical atom X. a Arrange the beakers in order of increasing concentration of X. b Without adding or removing X, what specific things could you do to make the concentrations of X equal in each beaker? (Hint: Think about dilutions.)SmartWork Ch. 16b Homework 1) Write the net ionic equation that rapresents what happens when sodium hydroxide dissolvas in water. If 0.0940 moles of sodium hydroxide were added to water, how many moles of OH would be produced? Number males OH 2) Which of the fallowing reactions would occur to a measurable extent in water? Cr aq) + H,O{) > HCl{aq) + OH"(aq) F"(aq) + H¿O() → HF(aq) + OH"(aq) Br (aç) + H2Ot) + HBrțaç) + OHT(aq) NH, (aq) + HzO + NH3(aq) + H30*(aq)