(a)
Interpretation: The solubility of
Concept introduction: The constant
(b)
Interpretation: The concentration of
Concept introduction: The constant
(c)
Interpretation: The concentration of
Concept introduction: The constant
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Chemistry: An Atoms First Approach
- Write equations for the stepwise formation of each of the following complex ions. a. CoF63 b. Zn(NH3)42+arrow_forwardA(NH3)3+ is a complex ion. A+(aq) + NH3(aq) ⇌ ANH3+(aq). K 1 = 3.3 x 10^3 ANH3+(aq) + NH3(aq) ⇌ A(NH3)2+(aq) K2 = 6.4 x 10^3 A(NH3)2+(aq) + NH3(aq) ⇌ A(NH3)3+(aq) K3 = 1.2 x 10^3 Calculate the equilibrium concentrations of all species in solution, including the spectator ions, NH4+, OH−, and H+, if 100.0 mL of 0.100 M ANO3 is added to 300.0 mL of 2.0 M NH3.arrow_forwardPredict if the following salts will increase, decrease or have no effect on the pH of an aqueous solution. MnCl4 K2SO4arrow_forward
- Bromothymol blue is yellow in acid solutions. HBB is acidic form of the indicator . The indicator is blue in basic solutions. BB- is basic form of the indicator. HBB + H2O H3O+ + BB- In this case, HBB is an acidic form of the indicator. BB- is the basic form of the indicator. The acidic form is yellow in color and the basic form is the blue color. (a) Predict what will happen if NaOH is added to the reaction system. explain why ? make sure to explain why?arrow_forwardCalculate the equilibrium concentration of Zn2+ in a 0.30-M solution of Zn(CN)4 2−.arrow_forwardWe have seen an introductory definition of an acid: An acid is a compound that reacts with water and increases the amount of hydronium ion present. In the chapter on acids and bases, we saw two more definitions of acids: acompound that donates a proton (a hydrogen ion, H+) to another compound is called a Brønsted-Lowry acid, and a Lewis acid is any species that can accept a pair of electrons. Explain why the introductory definition is amacroscopic definition, while the Brønsted-Lowry definition and the Lewis definition are microscopic definitions.arrow_forward
- What is the concentration (in molarity) of H+, HCO3−, and CO32–, in a solution that is initially prepared as a mixture of 0.0100 M H2CO3 and 0.000010 M Na2CO3? (Carbonic acid is a weak diprotic acid where Ka1 is 4.20 x 10–5 and Ka2 is 2.00 x 10–6) a) [H+] at equilibrium = ? b) [HCO3-] at equilibrium = ? c) [CO32-] at equilibrium = ?arrow_forwardWrite the K expression for an aqueous solution of hypochlorous acid:arrow_forwardPlease calculate the [H+] in the following solution at 298 K: a) 0.1 mol·dm-3 NaOH;b) 0.1 mol·dm-3 HCN ( 25ºC). (HCN is a monoprotic acid and Ka= 4.9×10^-10 at 25ºC.) c) A mixture of 0.1 mol·dm-3 CH3COOH and 0.1 mol·dm-3 CH3COONa at 25ºC.(CH3COOH is a monoprotic acid and its Ka=1.8×10^-5 at 25ºC.)arrow_forward
- Weak Acids dissociate according to the following equation: HA(aq) + H2O(L) ⇌ H3O+ (aq) + A-(aq) In a lab experiment, a student needs to make a buffer solution with a pH of 6.870. If the pKa of the weak acid is 6.500, what ratio of conjugate weak base to acid is needed to make the buffer, I.e. what is the value of [A-/HA]? (Please provide your answer to 3 decimal places.)arrow_forwardShow by suitable net ionic equations that each of the following species can act as a Brønsted-Lowrybase:(a) HS−(b) PO43−(c) NH2−(d) C2H5OH(e) O2−(f) H2PO4−arrow_forwardWrite the chemical equation and the expression for the equilibrium constant, and calculate Kb for the reaction of each of the following ions as a base. (a) sulfate ion (b) citrate ionarrow_forward
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