Prepare a buffer by direct addition. Close Problem Consider how best to prepare one liter of a buffer solution with pH = 7.66 using one of the weak acid/conjugate base systems shown here. %3D Weak AcidConjugate Base Ка pka HC2O4¯ C2042- H2PO4 HPO42- HCO3 CO3²- 6.4 x 10-5 4.19 6.2 x 10-8 7.21 4.8 x 10-1110.32 How many grams of the potassium salt of the weak acid must be combined with how many grams of the potassium salt of its conjugate base, to produce 1.00 L of a buffer that is 1.00 M in the weak base? grams potassium salt of weak acid = %3D grams potassium salt of coniugate base =

QUESTION 4 Kb (NH3)-1.8 x 10-5 If we mix 20.0 ml of 0.40 M NH3 with 40.0 ml of 0.20 M HCL, the solution pH will be equal to notations) QUESTION S at equilibrium. (type your answer, do not use scientific Ka (HF) 7.2 x 104 Now we mix 15.0 ml of 0.24 M HF and 15.0 ml of 0.24 M NaOH. At equilibrium, the pH of the mixture will be equal to (type your answer, do not use scientific notations)

Buffer C: 100.0 mL at pH= 12.000, [conj.base] = 0.500 M conjugate acid: HPO4 ^2- conjugate base: PO4 ^3- require concentration (in M) =1.05 mass of solid necessary as source of conjugate acid: 14.9 g

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11. 0.0100 M solution of HCN has pH=5.7. What is K₂ value and pką?

4 9. 10 A solution is prepared at 25 °C that is initially 0.26M in methylamine (CH,NH,),a weak base with K, = 4.4 × 10¯*, and 0.24M in methylammonium chloride (CH,NH, CI). Calculate the pH of the solution. Round your answer to 2 decimal places. pH = 0 ? %3D Submit As Continue Terms of Use Privacy Center O 2022 McGraw Hill LLC. All Rights Reserved.