can u help? im not sure about my answers Question 6 2 pts A 50.0 mL...
A 10.0 mL sample of 0.75 M CH3CH2COOH(aq) is titrated with 0.30 M NaOH(aq) (adding NaOH to CH3CH2COOH). Determine which region on the titration curve the mixture produced is in, and the pH of the mixture at each volume of added base. K of CH3CH2COOH is 1.3 x 10-5. base Henderson-Hasselbalch equation: pH = pK+ log NaOH CH3CH2COOH Parta): 1) After adding 18.0 mL of the NaOH solution, the mixture is (Select) equivalence point on the titration curve. 2) The...
A 10.0 mL sample of 0.75 M CH3CH2COOH(aq) is titrated with 0.30M NaOH(aq) (adding NaOH to CH3CH2COOH). Determine which region on the titration curve the mixture produced is in, and the pH of the mixture at each volume of added base.Ka of CH3CH2COOH is 1.3 × 10−5.Henderson–Hasselbalch equation: p H = p K a + log [ b a s e ] [ a c i d ]Part a):1) After adding 18.0 mL of the NaOH solution, the mixture is ...
A 10.0 mL sample of 0.75 M CH3CH2COOH(aq) is titrated with 0.30 M NaOH(aq) (adding NaOH to CH3CH2COOH). Determine which region on the titration curve the mixture produced is in, and the pH of the mixture at each volume of added base. K of CH3CH2COOH is 1.3 x 10-5 Henderson-Hasselbalch equation: pH =pK+ log NaOH CH3CH2COOH Parta): 1) After adding 18.0 mL of the NaOH solution, the mixture is before the equivalence point on the titration curve. 2) The pH...
Question 6 1 pts A 10.0 mL sample of 0.25 M NH3(aq) is titrated with 0.20 M HCl(aq) (adding HCl to NH3). Determine which region on the titration curve the mixture produced is in, and the pH of the mixture at each volume of added acid. Ko of NH3 is 1.8 x 10-5 Henderson-Hasselbalch equation: pH = pka + log og HCI NH, NH3- Parta): 1) After adding 10 mL of the HCl solution, the mixture is (Select] the equivalence...
part 2 Thank you so much! A 50.0 ml sample of 0.50 M HCllaa) is titrated with 60.0 mL of 0.50 M NaOHaą) l mixture adding NaOH to HCI). Determine which region on the titration curve the produced is in, and the pH of the mixture. Assume that the volumes of the solutions are additive. NaOH . HCI 1) After adding the NaOH solution, the mixture is Select) equivalence point on the titration curve. 2) The pH of the solution...
1)A 10.0 mL sample of 0.25 M NH3(aq) is titrated with 0.20 M HCl(aq) (adding HCl to NH3). Determine which region on the titration curve the mixture produced is in, and the pH of the mixture at each volume of added acid.Kb of NH3 is 1.8 × 10−5.Henderson–Hasselbalch equation:Part a):1) After adding 10 mL of the HCl solution, the mixture is [ Select ] ["at", "before", "after"] the equivalence point on the titration curve.2) The pH of the solution after...
A 10.0 mL sample of 0.25 M NaOH(aq) is titrated with 15.0 mL of 0.10 M HCl(aq) (adding HCl to NaOH). Determine which region on the titration curve the mixture produced is in, and the pH of the mixture. Assume that the volumes of the solutions are additive. 1)After adding the HCl solution, the mixture is [select one](before, After, at) the equivalence point on the titration curve. 2)The pH of the solution after adding HCl is [select one](7.00,1.40,11.00,12.60).
assignment will be closed on Friday, March 29th at 12.00 PM (noon). The correct answers will be available on Friday March 29th. at 12:05 PM Question 1 1 pts A 10.0 mL sample of 0.25 M NHsloq) is titrated with 10.0 mL of 0.20 M HCloa) (adding HCI to NHal. Determine which region on the titration curve the mixture produced is in, and the pH of the mixture. Kb of NH3 is 1.8 × 10-5. Henderson-Hasselbalch equation: pH base] HCI...
A 10.0 mL sample of 0.75 M CH3CH2COOH(aq) is titrated with 18.0 mL of 0.30 M NaOH(aq) (adding NaOH to CH3CH2COOH). Determine which region on the titration curve the mixture produced is in, and the pH of the mixture. Ka of CH3CH2COOH is 1.3 \times × 10−5. Henderson–Hasselbalch equation: LaTeX: pH=pK_a+\log\frac{\left[base\right]}{\left[acid\right]} p H = p K a + log [ b a s e ] [ a c i d ] 2046 HW10 Q1-1.jpg 1) After adding the NaOH...
An acid-base titration is performed: 250.0 mL of an unknown concentration of HCl(aq) is titrated to the equivalence point with 36.7 mL of a 0.1000 M aqueous solution of NaOH. Which of the following statements is not true of this titration? A. At the equivalence point, the OH−concentration in the solution is 3.67×10−3 M. B. The pH is less than 7 after adding 25 mL of NaOH solution. C. The pH at the equivalence point is 7.00. D. The HCl...