PROBLEM: Calculate the pH during the titration of 40.00 mL of 0.1000M propanoic acid (HPr; Ka = 1.3x10-5) after adding the following volumes of 0.100OM NaOH: %3D (a) 0.00mL (b) 30.00mL (c) 40.00mL (d) 50.00mL
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- 14) 40 ml of 0.0900 HCI is diluted to 100 ml with water and titrated with 0.1000M NAOH. Calculate the pH after the addition of the following volume (ml) of the titrant added: (a) 0.00 (b) 10.00 (c) 18.00 (d) 30.00 (e) 35.95 (f) 36.00 (g) 36.05 (h) 40.00- What is the pH of each of the following solutions? (a) 0.35 M hydrochloric acid (b) 0.35 M acetic acid (c) 0.035 M acetic acid [Note that the approximate method used in Equation 2.15 will not give a good answer at low Ag.]Addition of the indicator methyl orange to an unknownsolution leads to a yellow color. The addition of bromthymolblue to the same solution also leads to a yellow color.(a) Is the solution acidic, neutral, or basic? (b) What is therange (in whole numbers) of possible pH values for the solution?(c) Is there another indicator you could use to narrowthe range of possible pH values for the solution?
- Tutorial Problem for Weak Base and Strong Acid You are given an Erlenmeyer flask containing 100.00 mL of 0.100 M B¯ and a buret containing 0.100M HCI. B¯ is a weak acid with a K of 5.9 x 10 º. Calculate the pH of the solution (to 2 decimal places) after titrating the following volumes of HCl: What is the pH after 0.0 mL HCI is added? 4.0 At this point no strong acid has been added, so you need to solve a weak base pH problem. What volume of HCI is added at the equivalence point (to 0.1 mL)? 49 mL What is the pH at the equivalence point? 49. At this point no strong acid or weak base remains, so you need to solve a weak acid pH problem for the weak base's conjugate acid. What is the pH after 50.0 mL HCl is added? 49 You are in the buffer region here. You need to find the relative ratio of [B-]/[HB]. Make sure to convert K, into K, before using the Henderson-Hasselbalch equation. a What is the pH after 150.0 mL HCI is added? 4.0/ You are in a region where both the weak conjugate acid and…A)write expressions for pH and pOH of (NH4) 2SO4 B)write expressions for pH and pOH of NH4OH(A) Which of the following is the strongest base? NH (B) (C) (D)
- What mass of HI should be present in 0.250 L of solution to obtain a solution with pH value of 2.85. (A) 1.8 g (B) 0.035 g (C) 0.045 g (D) 0.055 gWithout detailed calculation and RICE table, determine whether the following solutions are acidic or basic, buffer or not buffer. Explain your answers by identifying the major species and the dominate chemical reaction. (a) 1M NaCl + 1M HCl in equal amounts (b) 1M NH4Cl + 1M NH3 in equal amounts (c) 1M Na2C2O4 + 1M HCl in equal amounts (d) 2M H3PO4 + 3M NaOH in equal amountsWithout detailed calculation and RICE table, determine whether the following solutions are acidic or basic, buffer or not buffer.Explain your answers by identifying the major speciesand the dominate chemical reaction. (a)1M NaCl + 1M HCl in equal amounts (b)1M NH4Cl + 1M NH3in equal amounts (c)1M Na2C2O4+ 1M HCl in equal amounts (d)2M H3PO4+ 3M NaOH in equal amounts
- (not in excel) Calculate the pH after addition of 0.00, 5.00, 25.00, 45.00, 49.00, 50.00, 51.00 and 55.00 mL of 0.1000 M NaOH in the titration of 50.00 mL of (a) 0.1000 M pyridinium chloride. (b) 0.1000 M lactic acid.Without detailed calculation and RICE table, determine whether the following solutions are acidic or basic, buffer or not buffer. Explain your answers by identifying the major species and the dominate chemical reaction. (a) 1M NaCl + 1M HCl in equal amounts (b) 1M NH,Cl + 1M NH3 in equal amounts (c) 1M Na2C2O4 + 1M HCl in equal amounts (d) 2M H3PO4 + 3M NaOH in equal amountsCalculate the pH of the solution resulting from the addition of 20.0 mL of 0.100 M NAOH to 30.0 mL of 0.100 M HNO3. 16 (a) 1.35 (b) 1.70 (c) 1.95 (d) 2.52 (e) 2.80