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1. What is the pH of this buffer?
2. What is the pH of the buffer after 0.300 mol of H+ have been added?
3. What is the pH of the buffer after 0.120 mol of OH- have been added?
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- A chemistry graduate student is given 125. mL of a 1.50M diethylamine ((C,H, NH solution. Diethylamine is a weak base with K,=1.3 × 10 °. What mass (HIN %3D of (C,H5), NH,Br should the student dissolve in the (C,H,) NH solution to turn it into a buffer with pH =10.79? 2. You may assume that the volume of the solution doesn't change when the (C,H) NH, Br is dissolved in it. Be sure your answer has a unit symbol, and round 12 it to 2 significant digits. 10A 93.0 mL sample of 0.0100 M HIO4 is titrated with 0.0200 M LIOH solution. Calculate the pH after the following volumes of base have been added. (a) 14.4 mL pH = 2.57 (d) 47.4 mL pH = X X (b) 44.2 mL pH = (e) 78.1 mL pH = X X (c) 46.5 mL pH = X0.915g of KHP (204.22g/mol) was dissolved in 100ml of distilled water and titrated euth sodium hydroxide solution. 27.55ml titrant was needed to reach the equivalenec point. There is 0.00448 moles of KHP present in the sample. a) How many moles of sodium hydroxide are needed to neutralize each mole of KHP? b) Therefore, how many moles of NaOH were needed to neutralize the KHP sample? c)What is the molar concentration (mol/L) of the sodium hydroxide solution?
- 4. A solution prepared to be initially 1 M in NH3 and 0.5 M in HCl is (Kb for NH3 = 1.8 x 10¯5): (A) a solution with a pH less than 7 that is not a buffer solution (B) a buffer solution with a pH between 4 and 7 (C) a buffer solution with a pH between 7 and 10 (D) a solution with a pH greater than 7 that is not a buffer solution (E) a solution with a pH of 775. pK, of NH," is 9.26. Hence, effective pH range for NH,OH-NH,Cl buffer is about :- (1) 8.26 to 10.26 (2) 4.74 to 5.74 (3) 3.74 to 5.74 (4) 8.26 to 9.26B ONLY (a)How many ml of 0.5 M HCl must be added to 100.0 ml of a 0.2 M Imidazole (C3H4N2 ; Kb=6.3x10-8) solution to obtain a pH of 5.52? (b)Is this solution a buffer?
- (f). Following are the titre values of two students when 25 mL of KIO3(aq) is titrated against Na2S2O3(aq).Titration no. Student 1 Student 21 2 3 24 24.9 25.7 25 24.1 24.0Which student is best in doing titration and why do you say so?(g). Taking the values of best student, calculate the concentration of the solution for which molarity is not known.(Note: first calculate moles of pipet solution in 25 mL, then moles of I2 and then moles of solution of unknown concentration and then its molarity by using average titre)Which solution is a buffer?(a) a solution that is 0.100 M in HNO2 and 0.100 M in HCl(b) a solution that is 0.100 M in HNO3 and 0.100 M in NaNO3(c) a solution that is 0.100 M in HNO2 and 0.100 M in NaCl(d) a solution that is 0.100 M in HNO2 and 0.100 M in NaNO2In the experiment conducted to determine the amount of acetic acid in vinegar, 8.2 mL of NaOH standard solution adjusted to 0.098 M was spent besides the phenolphthaleley indicator. Accordingly, which of the following is the amount of acetic acid in the vinegar sample in grams? (Ma (CH3COOH): 60.05 g/mol) A. 0.048 B. 0.024 C. 0.096 D.0.072
- 7) The POH of a buffer solution that is 0.080 M aqueous HF acid and 0.042 M NH,F is: (K, of HF = 5.40 x 104) a) 11.0 b) 9.56 c) 2.99Calculate the pH at the equivalence point in titrating 0.084 M solutions of each of the following with 0.078 M NAOH. (a) hydrobromic acid (HBr) pH = 2.52 (b) hydrosulfuric acid (H,S), K, = 9.5e-08 pH = 7.05 (c) phenol (HCsHş0), K, = 1.3e-10 pH =In the experiment conducted to determine the amount of acetic acid in vinegar, 8.2 mL of NaOH standard solution adjusted to 0.098 M was spent besides the phenolphthaleley indicator. Accordingly, which of the following is the amount of acetic acid in the vinegar sample in grams? (Ma (CH3COOH): 60.05 g / mol)