Lab9. Determine the Formation Constant of a Coordination Complex

For the aqueous [Ag (NH3)₂ complex K₁=1.12 × 107 at 25 °C. + Suppose equal volumes of 0.0042M AgNO3 solution and 0.86M NH3 solution are mixed. Calculate the equilibrium molarity of aqueous Ag ion. Round your answer to 2 significant digits. M x10 Times 10 to an exponent

How the aqueous chemistry of amphoteric hydroxides involves precipitation, complex-ion formation, and acid-base equilibria

A weak acid, HA, has a pKa = 6.2.  If a solution of NaA(aq) is prepared, what does the pH of the solution need to be adjusted to in order to achieve the following ratios of deprotonated to protonated species? 1) [A-] / [HA] = 0.01 2) [A-] / [HA] = 10 3) [A-] / [HA] = 1 4) [A-] / [HA] = 106 Note: NaA is the sodium salt of , the conjugate base of HA.  Assume NaA completely dissociates in water.

You've just started your summer intern as a research assistant in the biology department. Your first assignment is to prepare a pH 7.50 phosphate buffer solution to be used in the isolation of DNA from a cell culture. You've discovered the following items available to you in the lab: 0.514M HPO 4 (K a-4.2x10 13) 48.6 g KOH (molar mass 56.1g) a. Calculate the pH of your buffer. b. Do you think that this would be a suitable buffer? Explain. SHOW YOUR WORK. Upload your file here.

In aqueous solution the Ag ion forms a complex with two cyanide anions. Write the formation constant expression for the equilibrium between the hydrated metal ion and the aqueous complex. Under that, write the balanced chemical equation for the last step in the formation of the complex. K₂ = ☐ Write the Last Step: Last Step: ☑ ロ→ロ

calculate the ph and poh of a solution that is 0.18 M in HC2H3O2 and .43 M in Mg(C2A3O2)2 where the Ki for HC2H3O2 is 1.8x10^-5

What is the equilibrium constant value for  NaC2H3O2 and how do you find its Kb?

Write the balanced chemical equation associated with the formation constant, Kf , for each complex ion. Include phase symbols. Ag(CN)2−:   −⇀↽−↽−−⇀   BeF_(4)^(2)−:   −⇀↽−↽−−⇀

Consider the following expression for the equilibrium constant that represents the dissociation of iodic acid into hydronium and iodate ions. Ka [H3O+] [103] [HIO3] = = 0.161 When 176 g of iodic acid is dissolved in water to give an aqueous solution with a final volume of 1.00 L. Calculate the % dissociation of iodic acid to form iodate anions. The molar mass of iodic acid is 175.91 g mol-¹. a. 0.161% b.16.1% OC. 32.8% Od. 40.1% e. 83.9%

containing a complex ion. In the presence of excess OH', the Al3+ (aq) ion forms a hydroxide complex ion, Al(OH)4. Calculate the concentration of free Al³+ ion when 1.64x10-2 mol Al(CH3COO)3(s) is added to 1.00 L of solution in which [OH ] is held constant (buffered at pH 12.40). For Al(OH)4", K = 1.1x1033. ma [A1³+] = M

You have been contracted to determine how different salts affect the pH of water. Which of the solids in the following set should you test to investigate for the effects of cations on pH? Rb₂SO3 RbBrO AlBra CH3NH₂Br M9Cz

23. lodide ion (1) is the conjugate base of hydroiodic acid (HI). Why doesn't sodium iodide cause an appreciable increase in the pH of water when it dissolves into Na* and I ions? (a) The Na' is acidic and neutralizes the basicity of I (b) It is a stronger acid than it is a base in water, so Nal actually lowers the pH when dissolved. (c) There are no H₂O* ions present in the solution that could react with I. (d) At least a small amount of HI must be present in order for I to act as a base to raise the pH. (e) HI is a strong acid that reacts completely, which makes I a correspondingly weak base. 24. K, for methylamine (CH3NH₂) is the equilibrium constant for which reaction? (a) CHÍNH, + HO - CHÍNH + HO CH₂NH3 + OH* = CHÍNH + H2O CH₂NH™ + H₂O (b) CH₂NH₂ + H₂O (C) CHÍNH, + HO (d) CH₂NH₂ + OH (e) None of the above

The formation constant for FeY2−  is 1014.30. Calculate the concentration of free Fe2+ in a 0.560 M FeY2− solution at pH 10.0. At this pH, the value of ?Y4−  = 0.30.   [Fe2+] = ?M

Write the net ionic equation for the equilibrium that is established when calcium cyanide is dissolved in water. It is not necessary to include states such as (aq) or (I). This solution is V + H₂O +

Using the dissociation constant, Kd = 1 × 10–44, calculate the equilibrium concentrations of Fe3+ and CN– in a 0.333 M solution of Fe(CN)6 3−.

We dissolve 2.77 g of an unknown acid, HA, in enough water to produce 25.0 mL of solution. The pH of this solution of HA(aq) is 1.33. We titrate this solution with a 0.250 M solution of NaOH. It takes 41.8 mL of the NaOH solution to reach the equivalence point. (a)  What is the molar mass of HA? (b)  What is the pKa value of HA(aq)? (c) What is the pH at the equivalence point? (d) What is the pH one third along the titration when you still have twice as much HA(aq) as A-(aq)?

The first step in the preparation of magnesium metal is the precipitation of Mg(OH)2 from sea water by the addition of Ca(OH)2. The concentration of Mg2+(aq) in sea water is 5.37 × 10–2 M. Calculate the pH at which [Mg2+] is diminished to 1.0 × 10–5 M by the addition of Ca(OH)2.

Which salt would you expect to dissolve readily in acidic solution, calcium phosphate, Ca3(PO4)2, or calcium sulfate, CaSO4? Give an explanation.

Consider the insoluble compound zinc cyanide, Zn(CN)2. The zinc ion also forms a complex with ammonia . Write a balanced net ionic equation to show why the solubility of Zn (CN)2 (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Zn(NH3)4²+, K₁ = 2.9×10⁹. Be sure to specify states such as (aq) or (s). K = + Submit Answer + Retry Entire Group 1 more group attempt remaining

Calculate the equilibrium concentration of Zn2+(aq) in a solution that is initially 0.150 M Zn(NO3)2 and 0.800 M NH3.   The formation constant for [Zn(NH3)4]2+(aq) is Kf = 2.8 × 109.

For the aqueous [Hg14] complex K, -6.76 × 1029 at 25 °C. 2+ Suppose equal volumes of 0.0092 M Hg (NO3), solution and 0.80M NaI solution are mixed. Calculate the equilibrium molarity of aqueous Hgion. Round your answer to 2 significant digits. ? 00 Ом x10 × Ar

For the aqueous [Ag (CN)₂] complex K₁=1.26 × 10²¹ at 25 °C. + Suppose equal volumes of 0.0026M AgNO3 solution and 0.38M KCN solution are mixed. Calculate the equilibrium molarity of aqueous Agion. Round your answer to 2 significant digits. M ? ☐x10 × Ś

Explain how the dichromate-chromate equilibrium (eqn. 2) shifts in response to an increase or decrease in OH- ions. Express this in words and as an equation.