Determine the ionic strength of each of the following solutions:
a) 0.05M MgCl2 =
b) 0.05M NaCl =
c) 0.05M NaOH plus 0.05M MgCl2 (all in the same solution) =
d) 0.05M K2SO4 =
e) Water that is pH 2 from addition of HCl =
Determine the ionic strength of each of the following solutions: a) 0.05M MgCl2 = b) 0.05M...
Question #2 determine the ionic strength of each of the following solutions (a) 0.05 M MgCl2 ANS= (b) 0.05 M NaCI ANS= (c) 0.05 M NaOH plus 0.05 M MgCl2 (all in the same solution) ANS= (d) 0.05 M K2SO4 ANS= (e) water that is pH 2 from addition of HCI ANS=-
y Determine the ionic strength, 1, for each of the solutions. Assume complete dissociation of each salt and ignore any hydrolysis reactions. A solution of 0.00519 M NaOH. A solution of 0.00260 M CaBro. A solution of 0.000888 M HCl and 0.000767 M La(NO),
Determine the ionic strength, u, for each of the solutions. Assume complete dissociation of each salt and ignore any hydrolysis reactions. A solution of 0.00487 M NaOH = М A solution of 0.00253 M CuCl, M A solution of 0.000743 M HCI and 0.000640 M La(NO) =
Determine the ionic strength, ?μ, for each of the solutions. Assume complete dissociation of each salt and ignore any hydrolysis reactions. A solution of 0.00449 M FeSO30.00449 M FeSO3. ?= _________M A solution of 0.00227 M CaBr20.00227 M CaBr2. ?= _________M A solution of 0.000739 M HCl0.000739 M HCl and 0.000777 M NaBr0.000777 M NaBr. ?= _________M
2. Calculate the concentrations and activities of H3O+ for the following solutions (assume that the ionic strength is determined by the acid/base). Calculate the pH for each solution two ways: 1) pH = -log[H3O+] and 2) pH = -log @,0+. (a) 0.010 M HNO3 (b) 0.035 M KOH (c) 0.030 M HCI (d) 3.0 M HCI
Determine the ionic strength, ?μ, for each of the solutions. Assume complete dissociation of each salt and ignore any hydrolysis reactions. A solution of (0.000804 M Mg(NO3)2\) and 0.000443 M NaBr
Determine the ionic strength of the solution, the activity coefficients, and the activities of each ion in a solution containing 0.01 M (molar) NaCl, 0.005 M Ca(OH)2 and 0.01M MgSO4 I have solved for the ionic strength already but am stuck on calculating the activity coefficients! as well as the activity of each ion, Ionic strength = 0.065 M
4) Which of the following pH values indicate a neutral solution? (a) pH=2 (b) pH=5 (c) pH=7 (d) pH=9 5) Which of the following forms a solution with a pH of 13.7? (a)0.02M solution of NaOH (b) 0.04M solution of Mg(OH)2 (c) 0.2M solution of HCl (d) 0.5M solution of NaOH 6) Which of the following forms a solution with a pH of 13? (a) 0.01M solution of NaOH (b) 0.03M solution of HCl (c) 0.05M solution of Ba(OH)2 (d)...
20. When aqueous solutions of NaOH and MgCl2 are mixed, a precipitate forms. What is the correct formula for the precipitate? A) Mg(OH)2(8) B) NaCl(s) C) NaCl2(s) D) MgOH(s) E) MgCl2(8)
Please show work! i will rate Determine the ionic strength. u. for each of the solutions. Assume complete dissociation of each salt and ignore any hydrolysis reactions A solution of 0.00418 M HCI. A solution of 0.00135 M LaBr- A solution of 0.000873 M CaBr, and 0.000635 M Cuci, What is the activity coefficient for each ion at the given ionic strength at 25 °C? Activity coefficients at various ionic strengths can be found in this table. so ( =...