Write out the charge balance equation for the solution in question below:"What is the ionic strength of a solution that has 0.020 M K2SO4 and 0.018 M NaCl ? (Assumecomplete dissociation)"
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Write out the charge balance equation for the solution in question below:
"What is the ionic strength of a solution that has 0.020 M K2SO4 and 0.018 M NaCl ? (Assume
complete dissociation)"
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Solved in 2 steps
- Calculate the OH- concentration in solution when the maximum anount of Fe(OH)3 has dissolved, if its ksp= 2.7x10^-39. The molar mass of Fe(OH)3 is 106.87 g/mol. Include the correct units and sig figs in answerI want the answer for Q2Give typed full explanation not a single word hand written otherwise leave it
- Select the statement below that is correct regarding the behavior of strong acids. O A strong acid and its sodium salt can be used to form a buffer solution. OA 1.0 M solution of a monoprotic strong acid will require twice as much 1.0 M NaOH to neutralize it as a 1.0 M solution of a monoprotic weak acid. Strong acids are acids with a solution concentration of > 3 M. O Strong acids ionize completely in solution.What is the freezing point of a 0.60 M solution of K₂SO₄? Assume that the completely dissociates into ions in water, and that for every mole of particles in a liter of water, the freezing point decreases by about 1.9°C.Effect of a common ion in dissociation of weak electrolytes.
- The indicator ethyl orange is an acid with a Ka of 4.6 ✕ 10−5. In a 1.9 ✕ 10−4 M solution, it is red in acid and yellow in base. Calculate the pH range over which it goes from 14% ionized (red) to 86% ionized (yellow). (a) pH at 14% ionized (b) pH at 86% ionizedIn a brief explanation, explain how you could analyze HCO3 - in a particular solution by using the volatilization method.2.3 N OF 0.174mL NaHCO3 IS NEUTRALIZED BY 31.5mL OF HCl, WHAT IS THENORMALITY OF THE ACID?
- What is pOH of a solution consisting of 1.35 M NH3 and 2.08 M NH4NO3? K, of NH4 * is 5.8 x 10 10 0 4.94 0 494 0 9.0612) What is the Molar Mass (g/mol) of an unknown monoprotic weak acid if 648 mg of it requires 35.86 mL of 0.1221 M NaOH to titrate it to equivalence (aq., 25 oC)?Give detailed Solution with explanation