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- You want to make a buffer with a pH of 10.00 from NH4+/NH3. (a) What must the [ NH4+ ]/[ NH3 ]ratio be? (b) How many moles of NH4Cl must be added to 465 mL of an aqueous solution of 1.24 M NH3 to give this pH? (c) How many milliliters of 0.236 M NH3 must be added to 2.08 g of NH4Cl to give this pH? (d) What volume of 0.499 M NH3 must be added to 395 mL, of 0.109 M NH4Cl to give this pH?A buffer system is prepared by combining 0.603 moles of ammonium chloride (NH4CI) and 0.713 moles of ammonia (NH3). What will the solution pH be if 0.239 moles of the nitric acid (HNO3) is added to the solution. Nitric acid is a strong acid. The K₁ of ammonia is 1.8 x 10-5. (Two decimal places)A chemistry graduate student is given 300. mL of a 1.40M ammonia (NH, solution. Ammonia is a weak base with K, =1.8 × 10 °. What mass of NH, Br -5 should the student dissolve in the NH, solution to turn it into a buffer with pH =9.81? You may assume that the volume of the solution doesn't change when the NH,Br is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 4 significant digits. x10 Explanation Check Accessibili 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center MacBook Pro
- Draw the titration curves for the titrations of (a) a strong acid with a strong base, (b) a strong acid with a weak base, (c) a weak acid with a strong base and (d) a weak acid with a weak base. Make sure you label each of them properly (volume on x-axis and pH on the y-axis). Describe how you would determine the Ka for a weak acid from the titration curves.Assume you titrate 20.0 mL of 0.11 M NH3 with 0.10 M HCl. (a) What is the pH of the NH3 solution before the titration begins? (b) What is the pH of the equivalence point? (c) What is the pH at the midpoint of the titration? (d) Which indicator would you suggest to detect the equivalence point? (e) Calculate the pH of the solution after adding 5.00, 11.0, 15.0, 20.0, 22.0, and 25.0 mL of the acid. Combine this information with that from (a) through (c) and plot the titration curve.A chemistry graduate student is given 450. mL of a 0.50M methylamine (CH, NH,) solution. Methylamine is a weak base with K,=4.4 × 10 *. What mass of CH,NH,Br should the student dissolve in the CH,NH, solution to turn it into a buffer with pH = 10.96? You may assume that the volume of the solution doesn't change when the CH,NH,Br is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. olo x10 Ar Explanation Check © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility .........................................
- A chemistry graduate student is given 450. mL of a 1.10M methylamine (CH,NH,) solution. Methylamine is a weak base 4 with K- :4.4 × 10 What mass of CH,NH,Cl should the student dissolve in the CH,NH, solution to turn it into a buffer with pH = 10.14? You may assume that the volume of the solution doesn't change when the CH,NH,Cl is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. x10A buffer solution contains 0.486 M hydrocyanic acid and 0.298 M potassium cyanide (K₂ (HCN) If 0.0309 moles of sodium hydroxide are added to 125 mL of this buffer, what is the pH of the resulting solution? (Assume that the volume does not change upon adding sodium hydroxide) pH = = 4.00 × 10-¹0).You have 30.00 mL of a 0.250 M aqueous solution of the weak base (CH3)2NH (Kb= 7.40 x 10-4).This solution will be titrated with 0.250 M HCl. (a) How many mL of acid must be added to reach the equivalence point? (b) What is the pH of the solution before any acid is added? (c) What is the pH of the solution after 5.00 mL of acid has been added? (d) What is the pH of the solution at the equivalence point of the titration? (e) What is the pH of the solution when 35.00 mL of acid has been added?
- x A chemistry graduate student is given 125. mL of a 0.90M dimethylamine ((CH3)2NH) solution. Dimethylamine is a weak base with K = 5.4 × 10. What (CH),NH,CI should the student dissolve in the (CH), NH solution to turn it into a buffer with pH = 11.23? You may assume that the volume of the solution doesn't change when the (CH,),NH,CI is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.4 A chemistry graduate student is given 100. mL of a 0.50M methylamine (CH,NH,) solution. Methylamine is a weak base with K,=4.4 × 10 *. What mass of CH,NH,Cl should the student dissolve in the CH, NH, solution to turn it into a buffer with pH = 10.93? You may assume that the volume of the solution doesn't change when the CH,NH, Cl is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. olo Ar x10Q2: Calculate the pH of the following acid-base buffers. 100 mL of 0.025 M formic acid and 0.015 M sodium format [a]after adding 5.0 x 10 mole of HCl.[b] after adding 5.0 x 10 mol of NaOH. [K, = 1.77x 10 1 %3D