A buffer solution is made that is 0.492 M in H2CO3 and 0.492 M in KHCO3. If Kal for H2CO3 is 4.20 X 10-7, what is the pH of the buffer solution? pH = _______ Write the net ionic equation for the reaction that occurs when 0.141 mol HNO3 is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H3O  instead of H+ )

You have 1.5 liter of solution that is composed of 8.88 grams of NH3 and 11.33 grams of ammonium chloride mixed well. Kb for ammonia =1.8 x 10^-5 (A) is this a buffer solution? Why or why not? (B)if it is a buffer solution, what is the pH of this buffer solution? (C)how many mL of 1.50 M HCl can be added to this solution before the buffer is exhausted (d) how many mL of 1.5 M NaOH can be added to this solution before the buffer is exhausted?

Write the buffer equilibrium reaction, then write the neutralization reaction. What isthe pH of the 0.20M NH3/NH4CL buffer after the addition of 10.0 mL of 0.10 HCl to65.0 mL of buffer? The Ka for NH3 is 5.6 x 10-10

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 .........................................