CONSIDER THE LACTIC ACID BUFFER WITH LACTIC ACID), CH₂CH(OH) COOH AND ITS SALT SODIUM LACTATE, CH₂CH(OH) COO Na ++₂0= -ott Ott

Buffer capacity is a measure of a buffer solution's resistance to changes in pH as strong acid or base is added. Suppose that you have 145 mL of a buffer that is 0.300 M in both acetic acid (CH₂COOH) and its conjugate base (CH3COO-). Calculate the maximum volume of 0.170M HCl that can be added to the buffer before its buffering capacity is lost. volume: esc ! 1 ← 2 #3 с $ 4 G Search or type URL 27 20 % MacBook Pro 5 ^ 6 & 7 +00 8 ( 9 ) mL 0 1

Three buffers are prepared with equal concentrations of formic acid and sodium formate (Buffer 1), hydrofluoric acid and sodium fluoride (Buffer 2), and acetic acid and sodium acetate (Buffer 3). Rank the three buffers from highest to lowest pH at which they can buffer a solution (i.e., their buffering pH).(a) 1, 2, 3(b) 3, 2, 1(c) 2, 1, 3(d) 3, 1, 2

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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)

Weak Acids dissociate according to the following equation: HA(aq) + H2O(L) ⇌ H3O+ (aq) + A-(aq) In a lab experiment, a student needs to make a buffer solution with a pH of 6.870.  If the pKa of the weak acid is 6.500, what ratio of conjugate weak base to acid is needed to make the buffer, I.e. what is the value of [A-/HA]? (Please provide your answer to 3 decimal places.)