gnment Score: 30.4% Resources Hint Check Ans cion 22 of 23 > For the titration of...
For the titration of 60.0 mL of 0.300 M NH3 with 0.500 M HCl at 25 °C, determine the relative pH at each of these points Determine the relative pH before the addition of any HCl pH 7 pH7 pH 7 Determine the relative pH after 36.0 mL HCl has been added. pH 7 pH7 pH 7 Determine the relative pH after 56.0 mL HCl has been added. pH 7 pH 7 pH = 7
7. In the titration of 10.0 mL of 0.500 M NH3 with 0.5 M HCI, calculate the pH of the following and sketch the titration curve. Kb 1.8 x 10 f. Before the titration starts g. After addition of 2.5 ml of HCl h. After addition of 5.0 ml of HCI i. After addition of 10.0 ml of HC
1 . If a buffer solution is 0.260 M in a weak acid (?a=8.3×10−5)and 0.480 M in its conjugate base, what is the pH? pH= 2. If a buffer solution is 0.200 M in a weak base (?b=5.0×10−5) and 0.530 M in its conjugate acid, what is the ph 3. Phosphoric acid is a triprotic acid (?a1=6.9×10−3, ?a2=6.2×10−8 , and ?a3=4.8×10−13 To find the pH of a buffer composed of H2PO4 - (aq) ) and HPO4 2− (aq) , which...
Determine the pH at the point in the titration of 40.0 mL of 0.200 M HC₄H₇O₂ with 0.100 M Sr(OH)₂ after 100.0 mL of the strong base has been added. The value of Ka for HC₄H₇O₂ is 1.5 × 10⁻⁵. HC4H7O2 (aq) + OH- --> H2O (l) +C4H7O2-
In the titration of a 25 mL of 0.245 M weak base (Kb = 1.76*10^-5) being titrated by 0.365 M HCl determine the following: a. The PH at the initial point b. The PH after 12.3 mL of HCl has been added c. The PH at the equivalence point d. The PH after 18.4 mL of HCl has been added
Assignment Score: 3450/5000 Resources 9 Hint Check Answer Question 8 of11 The pK, of hypochlorous acid is 7.530. A 57.0 ml. solution of 0.118 M sodium hypochlorite (NaOCI) is titrated with 0.335 M HCI Calculate the pH of the solution after the addition of 7.41 ml. of 0.335 M HCİ Calculate the pli of the solution after the addition of 20.9 ml. of 0.335 M HC the phi of the solution after the addition of 20.9 ml. of 0.335 M...
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Question 13 of 20 > Consider a titration of 50.0mL sample of 0.500 M HCl (a strong acid, which contains 0.0250 moles H:07) with 0.400 M NaOH (a strong base). Determine the pH of the solution after 15.0 mL of NaOH (0.00600 moles of OH) is added.
Assume a temperature of 25 'C for the following problems. 1. A titration of 20.00 mL of 0.275 M HCl is completed with 0.500 M KOH. Make sure your answers reflect the correct number of significant figures. For log rules and significant figures, review CHEMActivity 43. (Chapter 16, pH on the top of page 127 of your workbook). A) What is the volume of KOH required to reach the equivalence point? (B) What is the initial pH (before any base...
14 of 18 Questions Assignment Score: 60.2% Resources Hint Check Answer 100% Question 14 of 18 > 10 Question 1ofAllempls Correct The pki, values for the dibasic base B are pKb = 2.10 and pK 12 = 7.66. 046 11 Question O of o Attempts Calculate the pH at each of the points in the titration of 50.0 mL of a 0.70 M B(aq) solution with 0.70 M HCl(aq). What is the pH before addition of any HCI? 95% 12...
CHomework Chapter 17 Plotting a Titration Curve for a Carbonate-Bicarbonate System 9 of 24> Carbonic acid (H2COa) is a weak diprotic acid with K4.43 x 10-7 and K 4.73 x 10-11 change, and equilibrium values for each species and plugging these into the equlibrium constant expression. The expression HCO as shown in the equation using the equation Salts of the bicarbonate ion, such as sodium During the titration before the equivalence point, provided that the concentration of acid is significantly...