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Answered: - EASE SHOW A LOT OF WORK! THANK YOU! I know these are a lot

EASE SHOW A LOT OF WORK! THANK YOU! I know these are a lot and I can increase the price!!?

1.The observed solubility of the salt MX in 4.0?M?strong acid is 2.30 x?10^{?3}?M.? The?K_{a}?value for the acid HX is 1.00 x?10^{?9}.? Calculate the value of?K_{sp}?for the salt MX.

2.Consider a solution made by mixing 500.0 mL of 4.0?M?NH_{3}?and 500.0 mL of 0.40?M?AgNO_{3}. Ag^{+}?reacts with NH_{3}?to form AgNH_{3}^{+}?and Ag(NH_{3})_{2}^{+}:

Ag^{+}?+ NH_{3}??AgNH_{3}^{+} | K_{1}?= 2.1 x?10^{3} |

AgNH_{3}^{+}?+ NH_{3}??Ag(NH_{3})_{2}^{+} | K_{2}?= 8.2 x?10^{3} |

The concentration of Ag(NH_{3})_{2}^{+}?at equilibrium is____?

3.Given the following values of equilibrium constants:

Cu(OH)_{2}(s)??Cu^{2+}(aq) + 2OH^{?}(aq) | K_{sp}?= 1.6 x?19^{?19} |

Cu(NH_{3})_{4}^{2+}(aq)??Cu^{2+}(aq) + 4NH_{3}(aq) | K?= 1.0 x?10^{?13} |

^{}What is the value of the equilibrium constant for the following reaction?

????????? Cu(OH)_{2}(s) + 4NH_{3}(aq)??-->Cu(NH_{3})_{4}^{2+}(aq) + 2OH^{?}(aq)

4.Calculate the molar concentration of uncomplexed Zn^{2+}?in a solution that contains 0.20 mol of Zn(NH_{3})_{4}^{2+}per liter. The overall?K_{f}?for Zn(NH_{3})_{4}^{2+}?is 3.8 x?10^{9}.

5.

A 50.0-mL sample of 2.0 x?10^{?4}?M?CuNO_{3}?is added to 50.0 mL of 4.0?M?NaCN. Cu^{+}?reacts with CN^{?}?to form the complex ion Cu(CN)_{3}^{2?}:

Cu(CN)_{3}^{2?}??Cu^{+}?+ 3CN^{?} | K?= 1.0 x?10^{?9} |

Calculate the solubility of CuBr(s) (K_{sp}?= 1.0 x?10^{?5}) in 1.0 L of 1.0?M?NaCN.

PLEASE SHOW WORK!!?

1.? A 100. mL sample of 0.10 M HCl is mixed with 50. mL of 0.11 M NH3. What is the resulting pH? (Kb for NH3 = 1.8 x 10^-5)

2.?After adding 25.0 mL of 0.100?M?NaOH to 100.0 mL of 0.100?M?weak acid (HA), the pH is found to be 5.90.? Determine the value of?K_{a}?for the acid HA.

3.For carbonic acid (H_{2}CO_{3}),?K_{a1}?= 4.30 x?10^{?7}?and?K_{a2}?= 5.62 x?10^{?11}. Calculate the pH of a 0.50?M?solution of Na_{2}CO_{3}.

PLEASE SHOW WORK!!?

1.? A 100. mL sample of 0.10 M HCl is mixed with 50. mL of 0.11 M NH3. What is the resulting pH? (Kb for NH3 = 1.8 x 10^-5)

2.?After adding 25.0 mL of 0.100?M?NaOH to 100.0 mL of 0.100?M?weak acid (HA), the pH is found to be 5.90.? Determine the value of?K_{a}?for the acid HA.

3.For carbonic acid (H_{2}CO_{3}),?K_{a1}?= 4.30 x?10^{?7}?and?K_{a2}?= 5.62 x?10^{?11}. Calculate the pH of a 0.50?M?solution of Na_{2}CO_{3}.

4.Calculate the pH when 200.0 mL of a 1.00M?solution of H_{2}A (K_{a1}= 1.0 x?10^{?6},?K_{a2}= 1.0 x?10^{?10}) is titrated with the following volumes of 1.00MNaOH.

150.0 mL of 1.00MNaOH

5.Consider the titration of 200.0 mL of a 0.100?M?solution of the weak acid H_{2}A with 0.200?M?NaOH.? The first equivalence point is reached after 100.0 mL of 0.200?M?NaOH has been added, and the pH is 6.27.? The pH, after 65.0 mL of 0.200?M?NaOH has been added, is 4.95.

Calculate the value of?K_{a1}?for H_{2}A.

Thank you!!

4.Calculate the pH when 200.0 mL of a 1.00M?solution of H_{2}A (K_{a1}= 1.0 x?10^{?6},?K_{a2}= 1.0 x?10^{?10}) is titrated with the following volumes of 1.00MNaOH.

150.0 mL of 1.00MNaOH

5.Consider the titration of 200.0 mL of a 0.100?M?solution of the weak acid H_{2}A with 0.200?M?NaOH.? The first equivalence point is reached after 100.0 mL of 0.200?M?NaOH has been added, and the pH is 6.27.? The pH, after 65.0 mL of 0.200?M?NaOH has been added, is 4.95.

Calculate the value of?K_{a1}?for H_{2}A.

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