1
answer
0
watching
288
views
16 Nov 2019
Use information from Appendix D of your text to calculate the pH 0f a. 50.0 mL of 0.15 M HCOOH (formic acid) with 75.0 mL of 0.13 M sodium formate (HCOONa). b. 125.0 mL of 0.10 M NH_3 with 250.0 mL of 0.10 M NH_4Cl. A 250.0-mL buffer solution is 0.250 M in acetic acid (CH_3COOH) and 0.250 M sodium acetate (CH_3COONa) in 1.20 L. (K_a: 1.3 times 10^-5) a. What is the initial pH of this solution? b. What is the pH of the buffer after the addition 0.0050 mol of HCI? c. What is the pH of the buffer after the addition of 0.0050 mol of NaOH? Calculate the pH in the titration of 50.0 mL of 0.120 M acetic acid (CH_3COOH) by 0.240 M sodium hydroxide (NaOH) after the addition of (a) 10.0 mL of base, (b) 25.0 mL of base, and (c) 35.0 mL of base As a result of mineral erosion and biological activity, phosphate ion is common in natural waters, where it often precipitates as insoluble salts, such as Ca_3(PO_4)_2. If [Ca^2+] = [PO_4^3-] = 1.0 times 106-7 M in a given river will Ca_3(PO_4)_2 precipitate? K_sp of Ca_3(PO_4)_2 is 1.2 times 10^-29 To improve the quality of x-ray images used in the diagnosis of intestinal disorders, the patient drinks an aqueous suspension of BaSO_4 before the x-ray procedure. The Ba^2+ in the suspension is opaque to x-ray, but toxic; thus, the Ba^2+ is lowered by the addition of dilute Na_2SO_4. What is the solubility of BaSO_4 in (K_sp: 1.1 times 10^-10) in (a) pure water and in (b) 0.20 M Na_2SO_4? A saturated solution of Mg (OH)_2 in water has a pH of 10.38. Estimate the K_sp for this compound.
Use information from Appendix D of your text to calculate the pH 0f a. 50.0 mL of 0.15 M HCOOH (formic acid) with 75.0 mL of 0.13 M sodium formate (HCOONa). b. 125.0 mL of 0.10 M NH_3 with 250.0 mL of 0.10 M NH_4Cl. A 250.0-mL buffer solution is 0.250 M in acetic acid (CH_3COOH) and 0.250 M sodium acetate (CH_3COONa) in 1.20 L. (K_a: 1.3 times 10^-5) a. What is the initial pH of this solution? b. What is the pH of the buffer after the addition 0.0050 mol of HCI? c. What is the pH of the buffer after the addition of 0.0050 mol of NaOH? Calculate the pH in the titration of 50.0 mL of 0.120 M acetic acid (CH_3COOH) by 0.240 M sodium hydroxide (NaOH) after the addition of (a) 10.0 mL of base, (b) 25.0 mL of base, and (c) 35.0 mL of base As a result of mineral erosion and biological activity, phosphate ion is common in natural waters, where it often precipitates as insoluble salts, such as Ca_3(PO_4)_2. If [Ca^2+] = [PO_4^3-] = 1.0 times 106-7 M in a given river will Ca_3(PO_4)_2 precipitate? K_sp of Ca_3(PO_4)_2 is 1.2 times 10^-29 To improve the quality of x-ray images used in the diagnosis of intestinal disorders, the patient drinks an aqueous suspension of BaSO_4 before the x-ray procedure. The Ba^2+ in the suspension is opaque to x-ray, but toxic; thus, the Ba^2+ is lowered by the addition of dilute Na_2SO_4. What is the solubility of BaSO_4 in (K_sp: 1.1 times 10^-10) in (a) pure water and in (b) 0.20 M Na_2SO_4? A saturated solution of Mg (OH)_2 in water has a pH of 10.38. Estimate the K_sp for this compound.
Keith LeannonLv2
14 Sep 2019