Consider the following hypothetical dissociation:
(a) addition of A(NO3)3
(b) increase in temperature
(c) adding Na+, forming NaB
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Chemistry: Principles and Reactions
- Write an equation for an equilibrium system that would lead to the following expressions (ac) for K. (a) K=(Pco)2 (PH2)5(PC2H6)(PH2O)2 (b) K=(PNH3)4 (PO2)5(PNO)4 (PH2O)6 (c) K=[ ClO3 ]2 [ Mn2+ ]2(Pcl2)[ MNO4 ]2 [ H+ ]4 ; liquid water is a productarrow_forwardAt a temperature of 60 C, the vapor pressure of water is 0.196 atm. What is the value of the equilibrium constant KP for the transformation at 60 C? H2O(l)H2O(g)arrow_forwardConsider the system 4NH3(g)+3O2(g)2N2(g)+6H2O(l)H=1530.4kJ (a) How will the concentration of ammonia at equilibrium be affected by (1) removing O2(g)? (2) adding N2(g)? (3) adding water? (4) expanding the container? (5) increasing the temperature? (b) Which of the above factors will increase the value of K? Which will decrease it?arrow_forward
- Consider the equilibriumB(aq) + H2O(l) ⇌ HB+(aq) + OH-(aq).Suppose that a salt of HB+(aq)is added to a solution ofB(aq) at equilibrium. (a) Will the equilibrium constant forthe reaction increase, decrease, or stay the same? (b) Will theconcentration of B(aq) increase, decrease, or stay the same?(c) Will the pH of the solution increase, decrease, or staythe same?arrow_forwardThe equilibrium constant for the reaction N,O,(2) = 2NO,(8) is 6.10 x 10 ' at 25'C. Calculate the value of K for this reaction: NO,(g) = 1/2N,O4(g) (A) 327 (B) 164 (C) 12.8 (D) 3.05 × 10 ³ How many moles of HCOON must be added to 1.0 L of 0.10 M HCOOH to prepare a buffer solution with a pH of 3.4? (HCOOH K, = 2 × 10 “) (A) 0.01 (B) 0.05 (C) 0.1 (D) 0.2 What is the percent ionization of a 0.10 M solution of formic acid at 25°C? Formic acid, HCOOH, has a Ka value of 1.9 x 104 at 25°C. (A) 0.19% (B) 1.4% (C) 4.4% (D) 14%arrow_forwardHemoglobin (Hb) transports oxygen in the blood:HbH⁺(aq)+O₂(aq)+H₂O(l) →HbO₂(aq)+H₃O⁺(aq) In blood, [H₃O⁺] is held nearly constant at 4X10⁻⁸ M.(a) How does the equilibrium position change in the lungs?(b) How does it change in O₂-deficient cells?(c) Excessive vomiting may lead to metabolic alkalosis, in which [H₃O⁺] in blood decreases. How does this condition af-fect the ability of Hb to transport O₂?(d) Diabetes mellitus may lead to metabolic acidosis, in which [H₃O⁺] in blood increases. How does this condition affect the ability of Hb to transport O₂?arrow_forward
- Write the equilibrium constant expression, K, for the following reaction. Please enter the compounds in the order given in the reaction. If either the numerator or denominator is blank, please enter 1 CH3NH₂ (aq) + H₂O(1) ⇒ CH3NH3(aq) + OH-(aq) K =arrow_forwardThe dissociation of acetic acid, CH,COOH, has an equilibrium constant at 25°C of 1.8 x 10-5. CH,COOH(aq) = CH,COO-(aq) + H*(aq) If the equilibrium concentration of CH,COOH is 0.46 moles in 0.500 L of water and that of CH,CO is 8.1 x 10-3 moles in the same 0.500 L, calculate the concentration of H+ for the reaction.arrow_forward1. Write equilibrium constant expressions for the following reactions: 1a.) HCOOH(aq) ⇌ H+(aq) + HCOO–(aq) 1b.) 2HgO(s) ⇌ 2Hg(l) + O2(g) 2.) For the reaction I2(g) ⇌ 2I(g), Kc = 3.8 x 10–5 at 727°C. (a) What is Kc for the reverse reaction at this temperature? (b) Calculate Kc for the reaction ½I2(g) ⇌ I(g).arrow_forward
- For the reaction 4 PH; (g) = 6 H,(g) + P¿(g) the equilibrium concentrations were found to be [PH,] = 0.250 M, [H,] = 0.370 M, and [P] = 0.750 M. What is the equilibrium constant for this reaction? K.arrow_forwardMethanoic acid is also called formic acid. It has the chemical formula HCOOH(l). It is a colourless fuming liquid that is mainly used as a preservative. It exhibits the following equilibrium in water:HCOOH(aq) + H2O(l) → HCOO–(aq) + H3O+(aq) 4) The concentration of the hydroxide ion, OH-(aq), in an aqueous solution is 2.5 x 10–3 mol/L. What is the pH of the solution? PLEASE HELP THIS IS VERY URGENTarrow_forwardLactic acid, HC3H503, is responsible for the sour taste of old milk. At 25 °C, its Ka = 1.4 x 104. %3D (a) What is the Kb of its conjugate base, the lactate ion, C3H503? Kp = x 10 (b) Is its conjugate base a strong or weaker base than the acetate ion? weakerarrow_forward
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