Refer to the titration curve pictured below. What chemical species will be predominate in the sodium added? Be as specific as possible. 12 10 8 6 4 2 0.1 mM Na CH3COO™ Gradual pH change Water 75000

An aqueous solution contains 0.30 M ammonium bromide. One liter of this solution could be converted into a buffer by the addition of: (Assume that the volume remains constant as each substance is added.) 0.14 mol HCI O0.30 mol HCI O0.07 mol Ba(OH)2 0.29 mol NH3 0.29 mol CaBr2

Sketch an accurate titration curve by plotting pH as a function of mL of HCl added when a 40 mL solution of 0.100 M ammonia is titrated with 0.100 M HCl include pH values when:0mL of HCl is added, 10 mL, 20 mL, 30mL and 40 mL

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Which solution would be considered a buffer solution? 1) 0.50M NaF + 0.25M KF 2) 0.38M CH3COOH + 0.15M CH3COOH 3) 0.25M H2SO4 + 0.25M Na2SO4 4)1.25M LiNO3 + 0.50M HNO3 5) 0.50M NaCl + 0.50M HCl

4 Volume HCI Added (mL) Strong Base/Weak Acid Strong Acid/Strong Base Strong Acid/Weak Base Weak Acid/VWeak Base

A 25.0-mL sample of 0.30 M HCI is titrated with 0.30 M KOH. What is the pH of the solution after 3.3 mL of KOH have been added to the acid? Please report with 1 decimal place.

A buffer solution contains dissolved C6H5NH2 and C6H;NH3CI. The initial concentration of C6H5NH2 is 0.50 M and the pH of the buffer is 4.20. Determine the concentration of C6H5NH3* in the solution. The value of Kb for C6H5NH2 is 3.8 x 10 10. ( PREV 1 3 NEXT > Based on your ICE table and definition of Kb, set up the expression for Kb in order to determine the unknown. Do not combine or simplify terms. Kp 3.8 x 10-10 %3D %3D 5 RESET [0] [0.50] [x] [2x] [4.20] [6.3 x 10-5) [1.6 x 10-10] [3.8 х 1011 [x + 4.20] [x - 4.20] [x + 6.3 x 10-51 [x - 6.3 х 10-5] [x + 1.6 x 101°] [x - 1.6 x 10-10] [x + 3.8 x 10-101 [x - 3.8 x 101°]

Consider a solution of a weak acid  being titrated with a solution of a strong base to beyond the equivalence point. Which of the following statements is incorrect?   a. The pH will increase intially and then change very little until the equivalence point is reached   b. Only a small percentage of the weak acid will react with the added base   c. The volume of the base solution required to reach the equivalence point can be less than, equal to, or more than the volume of the acid solution.   d. At the equivalence point, the solution will be basic   e. Beyond the equivalence point, the solution will be basic   f. None of the above   g. The pH of the solution in the tiration flask is affected by the total volume at any given point

Please answer all 3 questions