What mass of ammonium nitrate must be added to 350 mL of a 0.150 M solution of ammonia to give a buffer having a pH of 9.00? (Kb(NH3) = 1.8 x 10-5)
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What mass of ammonium nitrate must be added to 350 mL of a 0.150 M solution of ammonia to give a buffer having a pH of 9.00? (Kb(NH3) = 1.8 x 10-5)
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- 5:50 1 Search Question 5 of 20 Submit Determine the mass of solid NaCH;COO that must be dissolved in an existing 500.0 mL solution of 0.200 M CH3COOH to form a buffer with a pH equal to 5.00. The value of Ka for CH-COОH is 1.8 х 10-5. 1 2 Let x represent the original concentration of CH;COO in the water. Based on the given values, set up the ICE table in order to determine the unknown. CH3COOH+ H20(1) =H;O*(aq) +CH3COO-(a Initial (M) Change (M) Equilibrium (M) 5 RESET 0.200 5.00 -5.00 1.0 x 10-9 -1.0 × 10-9 1.0 x 10-5 -1.0 x 10-5 1.8 x 10-5 -1.8 x 10-5 х+ 5.00 x - 5.00 x + 1.0 × 10-9 х - 1.0 х 10-9 1.0 x 10-5 x - 1.0 × 10-5 x + 1.8 × 10-5 х - 1.8 х 10-5Consider the reaction of a 20.0 mL of 0.220 M C₅H₅NHCl (Ka = 5.9 x 10⁻⁶) with 12.0 mL of 0.241 M CsOH. With 0.00151 moles of C₅H₅NH⁺ and 0.00289 moles of C₅H₅N in the beaker, what would be the pH of this solution after the reaction goes to completion and the system reaches equilibrium?A buffer is prepared by adding 4.8 g of (NH4)2SO4 to 425 mL of 0.258 M NH3. Assuming that the volume stays constant, what is pH of the buffer solution? Consider: Kb (NH3) = 1.8×10–5, and Molar Mass of (NH4)2SO4 = 132.14 g/mol. (A) 10.04 (B) 5.22 (C) 9.44 (D) 4.93 (E) 1.75
- Consider the reaction of a 20.0 mL of 0.220 M C₅H₅NHCl (Ka = 5.9 x 10⁻⁶) with 12.0 mL of 0.223 M CsOH. With 0.00172 moles of C₅H₅NH⁺ and 0.00268 moles of C₅H₅N in the beaker, what would be the pH of this solution after the reaction goes to completion and the system reaches equilibrium? please explain step by stepThe titration curve as shown is for the titration of 25.00 mL of 0.100 M CH3CO2H with 0.100 M NaOH. The reaction can be represented as: CH3 CO2 H + OH− ⟶ CH3 CO2− + H2 O(a) What is the initial pH before any amount of the NaOH solution has been added? Ka = 1.8 × 10−5 for CH3CO2H. (b) Find the pH after 25.00 mL of the NaOH solution have been added.(c) Find the pH after 12.50 mL of the NaOH solution has been added.(d) Find the pH after 37.50 mL of the NaOH solution has been added.4. A solution prepared to be initially 1 M in NH3 and 0.5 M in HCl is (Kb for NH3 = 1.8 x 10¯5): (A) a solution with a pH less than 7 that is not a buffer solution (B) a buffer solution with a pH between 4 and 7 (C) a buffer solution with a pH between 7 and 10 (D) a solution with a pH greater than 7 that is not a buffer solution (E) a solution with a pH of 7
- 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(a) Calculate the pH of a 0.500 L buffer solution composed of 0.700 M formic acid (HCOOH, Ka = 1.77 x 10-4) and 0.500 M sodium formate (HCOONa). (b) Calculate the pH after adding 50.0 mL of a 1.00 M NaOH solution.6. A buffer solution is formed by adding 0.500 mol of sodium acetate (CH3CO2NA) and 0.500 mol of acetic acid (CH3CO2H) to 1.00 L H,0. What is the pH of the solution at equilibrium? (K, = %3D 1.8 x 10°)
- Determine the pH of (a) A 0.10 M CH3COOH solution (ICE) (b) A solution that is 0.10 M CH3COOH and 0.10 M CH3COONa. Ka for CH3COOH = 1.8 X 10-5.Which of the following pairs of solution would you use to prepare a buffer with pH = 7.45? (A) Acetic acid + sodium acetate; (CH3CO2H has Ka = 1.8 x 10–5) (B) Sodium dihydrogen phosphate + sodium hydrogen phosphate; (H2PO4– has Ka = 6.2 x 10–8) (C) Ammonium chloride + ammonia; (NH3 has Kb = 1.8 x 10–5) (D) Sodium hydrogen carbonate + sodium carbonate; (HCO3– has Ka = 5.6 x 10–11)A buffer consists of 0.50 M NaH₂PO₄ and 0.40 M Na₂HPO₄.Phosphoric acid is a triprotic acid (Kₐ₁=17.2X10⁻³, Kₐ₂=26.3X10⁻⁸, and Kₐ₃=34.2X10⁻¹³). (a) Which Kₐ value is most important to this buffer? (b) What is the buffer pH?