Practice Exercise of precipitation titration: Calculate the titration curve for the titration of 50.0 mL of 0.0500 M AgNO, with 0.100 M NaCl 1) as pAg versus Nac 2) as pC1 versus Naci
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- Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a) before any NaOH is added? (b) at half-neutralization? (c) at the equivalence point? (d) when 0.10 mL less than the volume of NaOH to reach the equivalence point is added? (e) when 0.10 mL more than the volume of NaOH to reach the equivalence point is added? (f) Use your data to construct a plot similar to that shown in Figure 14.10 (pH versus volume NaOH added).Neutralization Titration In the standardization of HCI solution using 10.00 ml of 0.02 Na,co, according to the equation M of Na,CO, 2 HCI 2NaCl + H₂O+CO, 15.0 ml of HCI is required to reach the end point using Bromocresol green indicator the molarity of HCI (mol/L) would be al 0.032 b) 0.027 20.013 d) 0.008 e) 0.064A 22.0 mL sample of 0.124 mol L1 diprotic acid (H,A) solution is titrated with 0.1021 mol L- KOH. The acid ionization constants for the acid are Ka = 5.2 x 10-5 and K, = 3.4 x 10 10 Part A At what added volume of base does the first equivalence point occur? ? V = mL Submit Request Answer Part B At what added volume of base does the second equivalence point occur? V = mL Submit Request Answer
- ) Calculate pAg+ in a precipitation titration if 50.00 mL of 0.06 M Ag" solution is added to 22.00 mL of 0.12 M NaN3 AgN3(s) K= 2.8x109 ksp = [ ag'] [N]% KsP 0.06-005 X - 0.8 0.1-0.05 0.75-0.8n 0 The following pH curve is for the titration of 20.0 mL of a 0.10 M solution of a weak monoprotic acid with a 0.10 M solution of a strong monoprotic base. Data points at 1 mL increments. 14.0 12.0 10.0 Hd 8.0 6.0 4.0 2.0 0.0 0.0 10.0 20.0 ession# 188... 30.0 Volume of titrant (mL) 40.0 50.0When carrying out a precipitation volume, the concentrations of the reactive species must be calculated in the pre-equivalence region, equivalence point, and post-equivalence region. In this context, calculate the concentration of SCN- in the titrated solution during the titration of 50.00 mL of AgNO3 0.100 mol / L with KSCN 0.100 mol / L after adding 41.12 mL of the titrant solution Given: Kps (AgSCN) = 1.10.10-12 pSCN = ??
- For the titration of a strong acid with a strong base, which statement below is FALSE? O Past the equivalence point, the pH is due to diluted excess strong basest the equivalence point, the pH is due to diluted excess strong base O Between V =0 mL and the equivalence point, the pH is due to diluted unreacted strong acid. O At V = 0 mL titrant added, the pH is due to initial concentration of strong acid. O The indicator changes color at the end point due to excess acid. At the equivalence point, the pH is due to the auto-ionization of water.Question 19 of 25 The molar solubility of Mg(CN)2 is 1.4 x 10-5 M at a certain temperature. Determine the value of Ksp for Mg(CN). NEXT Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. Mg(CN) (s) Mg (aq) 2 CN-(aq) Initial (M) Change (M) Equilibrium (M) O RESET 1.4 x 105 -1.4 x 10-5 2.8 x 10-5 -2.8 x 10-5 +x +2x -2x 1.4 x 10-5 + x 1.4 x 10- + 2x 1.4 x 10-5 - x 1.4 x 10 - 2x 2.8 x 10-5 + x 2.8 x 10+ 2r -x 2.8 x 10-5 - x 2.8 x 10 - 2xCalculate the pH at different points as 25.0 mL of 0.20 M nitrous acid is titrated with 0.15 M sodium hydroxide. Ka (HNO2) = 4.5x10-4 a) Initial pH of the weak acid solution b) Volume of titrant at the equivalence point c) pH at the equivalence point d) pKa of the acid e) pH at two different points in the buffer region f) pH at two different points after the equivalence point
- Titration You are titrating 10 mL 0.050 M benzoic acid (pK, = 4.19) with 0.025 M sodium hydroxide.A buffer is made using 50.00 mL of 0.7000 M HA (a weak acid, Ką = 1.000 x 10-5) and 50.00 mL of 0.7000 M NaA. What volume (in units of liters) of 0.05000 M NaOH must be added to change the pH of the original buffer solution by 3.393 %. Answer: The correct answer is: 0.1350- 3 A chemistry graduate student is given 450. mL of a 0.30 M chloroacetic acid (HCH,CICO,) solution. Chloroacetic acid is a weak acid with K,= = 1.3 × 10 What mass of NaCH,CICO, should the student dissolve in the HCH,CICO, solution to turn it into a buffer with pH = 2.81? You may assume that the volume of the solution doesn't change when the NaCH,CICO, is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. x10