7 a A buffer solution is an aqueous solution consisting of a mixture of a weak acid and its conjugate base, or vice versa. so this option is incorrect
b. This is correct
From among c and d, d is correct, it is a direct consequence of the Hendersen-Hasselbach Equation.
8 The option d is wrong here. In a salt the cations move to the cathode to compensate for the loss of the cations during functioning of the electrochemicl cell. Similarly, anions move to the anode region.
9 a and d. "d" is the exact answer. "a" is the result of "d".
The equivalence point is the ideal point for the completion of titration. In order to obtain accurate results the equivalence point must be attained precisely and accurately. The solution of known concentration, or titrant, must be added to the solution of unknown concentration, or analyte, very slowly in order to obtain a good result. At the equivalence point the correct amount of standard solution must be added to fully react with the unknown concentration.
The end point of a titration indicates once the equivalence point has been reached. It is indicated by some form of indicator which varies depending on what type of titration being done.
9. b will show a higher quantum yield since it is structure is more rigid out of the two molecules
Which tement regarding buffer solution is correct? sobation is cemposod of a misture of a weak...
Can you answer this please and explain? 7. Which of the following regarding buffer is incorreer? a. Buffer pH depends on ionic strength and temperature b. B acid or base is added. er capacity is a measure of how well a solution resists changes in pH when strong c. You can make a buffer solution using a strong acid and a strong base olution to a weak acid You can make a buffer solution by adding a strong base s...
A pH 4 buffer solution is prepared by dissolving one mole of a weak acid HA (pKa=4) and one mole NaA in 1 L of water. When the volume is increased to 10L by adding distilled water, the pH of the resulting solution is closest to. 7.0 6.0 5.0 4.0 3.0
which weak acid would be best to use when preparing a buffer solution with a pH of 4.76? hypobromous acid chloroacetic acid propanoic acid nitrous acid
Which weak acid would be best to use when preparing a buffer solution with a pH of 8.40? an acid with pK, - 3.20 O an acid with pK= 5.10 O an acid with pK= 4.30 O an acid with pK= 9.60 an acid with pK, = 8.38 an acid with pKg = 6.20
Which weak acid would be best to use when preparing a buffer solution with a pH of 8.10? An acid with Ka = 5.0 × 10-10 An acid with Ka = 8.3 × 10-9 An acid with Ka = 1.6 × 10-5 An acid with Ka = 1.0 × 10-4 An acid with Ka = 1.3 × 10-6 An acid with Ka = 1.3 × 10-3
A buffer solution is able to maintain a constant pH when small amounts of acid or base are added to the buffer. Consider what happens when 1 mL of a 5 M solution is added or 0.005 mol of HCl are added to a 100.0 mL solution acetic acid buffer that contains 0.0100 mol of Acetic acid, HC,H,O,, and 0.0100 mol of sodium acetate, NaC,H,O,. The initial concentration of both the acid and the base are 0.0100 mol/ 0.1000 L...
Question two A buffer solution is able to maintain a constant pH when small amounts of acid or base are added to the buffer. Consider what happens when 1 mL of a 5 M solution is added or 0.005 mol of HCl are added to a 100.0 ml solution acetic acid buffer that contains 0.0100 mol of Acetic acid, HC,H,O,, and 0.0100 mol of sodium acetate, NaC,H,O2. The initial concentration of both the acid and the base are 0.0100 mol/0.1000...
Typical Math Problems 1) What is the pH of a buffer solution which is 0.12M in benzoic acid, pKa 4.19, and is 0.11M in sodium benzoate? 2) Find the %-diss of a buffer if the pKa 7.10 and the pH of the buffer is 7.50. 3) A weak monoprotic acid has a pKa 6.15. 50.00 mL of an 0.1250M aqueous solution of this weak acid is titrated with 0.1000M Na0H. a) What is the equivalence point volume and ½ equivalence...