Find the equilibrium concentration of the Mn(C2O4)22− ion(in M) when 0.50 L of 0.030 M Mn(NO3)2...

Find the equilibrium concentration of the Mn(C2O4)22− ion(in M) when 0.50 L of 0.030 M Mn(NO3)2 are mixed with 1.0 L of 1.2M Na2C2O4. Kf of Mn(C2O4)22− is 6.3 x 105.

What is the molar solubility of lead(II) chromate in 0.10 M Na2S2O3? For PbCrO4, Ksp = 2.0 x 10–16; for Pb(S2O3)34–, Kf = 2.2 x 106.

Expert Solution

queen_honey_blossom answered 2 years ago

Find the equilibrium concentration of the Mn(C2O4)2− ion(in M) when 0.50 L of 0.030 M Mn(NO3)2...

Find the equilibrium concentration of the Mn(C2O4)2− ion(in M) when 0.50 L of 0.030 M Mn(NO3)2 are mixed with 1.0 L of 1.2M Na2C2O4. Kf of Mn(C2O4)2 2- is 6.3 x 10 5.

A solution is 0.010 M in each of Pb(NO3)2, Mn(NO3)2, and Zn(NO3)2. Solid NaOH is added...

A solution is 0.010 M in each of Pb(NO3)2, Mn(NO3)2, and Zn(NO3)2. Solid NaOH is added until the pH of the solution is 8.50. Which of the following is true? Pb(OH)2, Ksp= 1.4 x10^-20 Mn(OH)2, Ksp= 2.0 x 10^-13 Zn(OH)2, Ksp= 2.1 x10^-16 A) No precipitate will form. B) Only Pb(OH)2 will precipitate. C) Only Mn(OH)2 wil precipitate. D) Only Zn(OH)2 and Pb(OH)2 will preipitate. E) All three hydroxide will preipitate.

Using the appropriate Ksp values, find the concentration of NO3− ions in the solution at equilibrium...

Using the appropriate Ksp values, find the concentration of NO3− ions in the solution at equilibrium after 700 mL of 0.35 M aqueous Cu(NO3)2 solution has been mixed with 350 mL of 0.40 M aqueous KOH solution. (Enter in M.) (Ksp for Cu(OH)2 is 2.6x10-19). Now find the concentration of OH− ions in this solution at equilibrium. (Enter in M.)

What is the equilibrium Mg2+ concentration when 1.75 L of a 0.153 M magnesium acetate solution...

What is the equilibrium Mg2+ concentration when 1.75 L of a 0.153 M magnesium acetate solution are mixed with 1.69 L of a 0.292 M ammonium carbonate solution? [Mg2+] =

A 1.00 L solution contains 5.00x106-5 M Cu(NO3)2 and 1.00x10^-3 M ethylenediamine. What is the concentration...

A 1.00 L solution contains 5.00x106-5 M Cu(NO3)2 and 1.00x10^-3 M ethylenediamine. What is the concentration of Cu2+ (aq) in the solution

What is the equilibrium concentration of ammonium ion in a 0.33 M solution of ammonia (NH3,...

What is the equilibrium concentration of ammonium ion in a 0.33 M solution of ammonia (NH3, Kb = 1.8 × 10–5) at 25oC? An initially 1.0 M aqueous solution of a weak monoprotic acid has a total ion concentration of M when equilibrium is established. What is the acid-ionization constant, Ka, of the weak acid? (assume Ca/Ka ≥ 102) For the reaction ΔG°700K = –13.457 kJ. What is Kp for this reaction at 700. K?

The equilibrium concentration of hydroxide ion in a saturated cobalt(II) hydroxide solution is ...................M.

Consider a 1.00 L, 1.00 M solution of NaNO3. Will the concentration of NO3- decrease, stay...

Consider a 1.00 L, 1.00 M solution of NaNO3. Will the concentration of NO3- decrease, stay the same, or increase if... A) half of the solution is poured out? B) 500 mL of water is added? C) 500 mL of 1.00M NaNO3 is added? D) 1.00 L of 0.500M NaNO3 is added? E) 1.00 L of 1.00 M NaCl is added? Please show work/explain reasoning

What is the equilibrium concentration of Ni^2+ (aq) in the solution. If one millimole of Ni(NO3)2...

What is the equilibrium concentration of Ni^2+ (aq) in the solution. If one millimole of Ni(NO3)2 dissolves in 220.0 mL of a solution that is 0.300 M in ammonia?

A solution is prepared by mixing 50.0 mL of 0.50 M Cu(NO3)2 with 50.0 mL of...

A solution is prepared by mixing 50.0 mL of 0.50 M Cu(NO3)2 with 50.0 mL of 0.50 M Co(NO3)2. Sodium hydroxide is then added to the mixture. Assume no change in volume. Ksp = 2.2 × 10-20 for Cu(OH)2, Ksp = 1.3 × 10-15 for Co(OH)2 The hydroxide concentration at which the first metal hydroxide will just begin to precipitate is __________M Using the integer designators, the metal hydroxide that precipitates first is {(1) Cu(OH)2 or (2) Co(OH)2 } _____________M...

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