A buffer solution contains 0.396MCH, NH, Br and 0.266MCH, NH, (methylamine). Determine the pH change when 0.063mol NaOH is added to 1.00% of the buffer. pH after addition -pH before addition pH change = A buffer solution contains 0.396 M CH3NH3Br and 0.266 M CH3NH2 (methylamine). Determine the pH change when 0.063 mol NaOH is added to 1.00 L of the buffer. pH after addition - pH before addition = pH change: =

Each symbol in the box below represents a mole of a component in one liter of a buffer solution; represents the anion (X-), = the weak acid (HX), = H+, and =OH. Water molecules and the few H+ and OH- ions from the dissociation of HX and X- are not shown. The box contains 10 mol of a weak acid, , in a liter of solution. Show what happens upon (a) the addition of 2 mol of OH- (2 ). (b) the addition of 5 mol of OH- (5 ). (c) the addition of 10 mol of OH- (10 ). (d) the addition of 12 mol of OH- (12 ). Which addition (a)-(d) represents neutralization halfway to the equivalence point?

Ka for formic acid is 1.7 104 at 25C. A buffer is made by mixing 529 mL of 0.465 M formic acid, HCHO2, and 494 mL of 0.524 M sodium formate, NaCHO2. Calculate the pH of this solution at 25C after 110 mL of 0.152 M HCl has been added to this buffer.

What is the pH of a buffer that is 0.150 M in a weak acid and 0.150 M in the acids conjugate base? The acids ionization constant is 6.8 106.