Exercise 11 (a) Calculate the molar concentrations of 1.00 ppm solutions each of Lit and Pb²+ Answer: Lit=1.44 x 104 M Pb²=4.83 x 10º M (a) What weight of Pb(NO3)2 will have to be dissolve in 1 liter of water to prepare a 100 ppm Pb2+ solution? Answer: 0.160 g 39
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- Exercise 2: A diprotic acid (H₂A) is titrated with NaOH to determine its molar mass according to the following equation: H₂A (aq) + 2 NaOH(aq) 2H₂O(1) + Na₂A (aq) Several experiments are performed by weighing a sample of H₂A, dissolve in water, with addition of few drops of phenolphthalein (ph.ph) indicator. The following data are obtained. Mass of H₂A Volume (mL) of 0.1M NaOH Molar mass of H₂A Average molar mass 46.5 55.5 0.22 0.28 0.30 0.32 0.25 0.28 Hint: mole H₂A=- UlSuppose you have equal volumes of saturated solutions of NaNO3, Na2SO4, and PbS. Which solution would dissolve the most lead(II) sulfate, PbSO4?The beaker on the left below represents a buffer solution of a weak acid HA and its conjugate base, A. (Water molecules and spectator ions have been omitted for clarity.) a Which beaker on the right, X or Y, depicts the solution after the addition of two formula units of NaOH? b How many HCl molecules can be added to the original buffer solution before the buffer capacity is exceeded? c Draw a picture of the solution where the buffer capacity has been exceeded by the addition of HCl.Check Your Understanding Calculate the molar solubility of silver cyanide. What does this correspond to in grams of solute per 100 grams of solvent? What assumptions must be made? Answer + 7.7 x 10-9 M 1.0 x 10- g/100 g H,OPractice Exercise of precipitation titration: Calculate the titration curve for the titration of 50.0 mL of 0.0500 M AgNO3 with 0.100 M NaCl 1) as pAg versus Naci 2) as pCl versus NaciKnowledge Check Question 12 A chemistry student weighs out 0.421 g of citric acid (H,C,H,O,), a triprotic acid, into a 250. mL volumetric flask and dilutes to the mark with distilled wate He plans to titrate the acid with 0.1900 M NAOH solution. Calculate the volume of NaOH solution the student will need to add to reach the final equivalence point. Be sure your answer has the correct number of significant digits. ml x10 I Don't Know Submit Terms of Use Pacy Act 02020 McGraw-Hill Education All Rightss Reserved PType here to searchEXERCISE 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…PROCEDURE 1000 mg L-asocrbic acid tablet (pulverized into fine powder) Molar mass of tablet = 176.12 g/mol 1. Add the necessary amount of distilled water to make the desired concentration of stock solution. [Note: Assume that the volume of the solute is negligible compared to the volume of the solution.] Concentration of STOCK SOLUTION, M Concentration of DILUTED SOLUTION, M 0.8 M 0.16 M 2. Mix and stir the powder with the distilled water until homogeneous. 3. Get ready for the dilution. Refer to the table above. 4. Compute and add more solvent to achieve the desired dilution. Use the prepared stock solution to prepare an aliquot assigned to your group. Make sure to place the computations used for dilution (C1V1 = C2V2) in the data sheet. 5. After dilution, label the aliquot with its concentration and total volume of solution. 6. Complete the data sheet with relevant solutions in solving for the amounts needed in the experiment. PLEASE FILL IN THE MISSING TABLES IN THE DATA…substrate dissolved in 0.15 M sodium phosphate solution, pH 6.2 and 1.40 mL of 0.15 M sodium phosphate, pH 6.2 solution. If the final volume of your test tube is 5.0 mL, what's your final concentration (M) of sodium phosphate in the tube? Your Answer: 0.042 Answer M unitsQUESTION 4 What is the hydronium ion concentration in a solution prepared by mixing 50.00 mL of 0.10 M HCN with 50.00 mL of 0.010M NaCN? Assume that the volumes of the solutions are additive and that Ka= 4.9 x 10 -10 for HCN. 7.0 x 10-6 M 4.9 x 10 M O 4.9 x 10-10 M 11 4.9 x 10 Click Save and Submit to save and submit. Click-Save All Answers to save all answers. Save All Ans MacBook Air DII DD 20 F8 F9 F10 F5 F6 F7 F3 F4 & %24 8. E A T. Y.EXERCISE II -10 1. Calculate the pH and the concentration of all species at the start of the titration of 0.100 M H3PO4 and 0.100 M NaOH. 2. Calculate the pH and the concentrations of all species halfway to the first equivalent point in the titration of 0.100 M H3PO4 and 0.100 M NAOH. 3. What is the pH of the carbonic acid if 20.00 mL of 0.0500 M H2CO3 is titrated with (a) 0.00 mL; (b) 10.00 mL ; (c ) 20.00 mL ; (d) 30.00 mL ; (e) 40.00 mL of 0.0500 M NAOH was added.PROCEDURE 1000 mg L-asocrbic acid tablet (pulverized into fine powder) Molar mass of tablet = 176.12 g/mol 1. Add the necessary amount of distilled water to make the desired concentration of stock solution. [Note: Assume that the volume of the solute is negligible compared to the volume of the solution.] Concentration of STOCK SOLUTION, M Concentration of DILUTED SOLUTION, M 0.8 M 0.16 M 2. Mix and stir the powder with the distilled water until homogeneous. 3. Get ready for the dilution. Refer to the table above. 4. Compute and add more solvent to achieve the desired dilution. Use the prepared stock solution to prepare an aliquot assigned to your group. Make sure to place the computations used for dilution (C1V1 = C2V2) in the data sheet. 5. After dilution, label the aliquot with its concentration and total volume of solution. 6. Complete the data sheet with relevant solutions in solving for the amounts needed in the experiment. PLEASE FILL IN THE MISSING TABLES IN THE DATA…SEE MORE QUESTIONS