Recent questions in Chemical equilibrium

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1 answer 34 views

Assuming that a 0.1 M solution of NH4Cl is at equilibrium with its own ions and NH3 in a closed vessel at 25°C. Calculate the effects on the equilibrium position when solid NH4Cl is added to the solution, and the final concentration of NH4+ and NH3 ions in the solution.

asked Jan 22 in Chemical equilibrium by RedaDoy9962 (410 points)

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1 answer 7 views

Assuming a chemical equilibrium reaction aA + bB ⇌ cC + dD, with initial concentrations of [A] = 0.2 M, [B] = 0.3 M, [C] = 0 M, and [D] = 0 M at 25°C, what will be the new equilibrium concentration of [B] if the volume of the container is decreased to half the original volume?

asked Jan 22 in Chemical equilibrium by JannieSerrat (990 points)

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1 answer 42 views

Assume a reaction has reached equilibrium in a 1-liter container. If the volume is now reduced to 0.5 liters, what is the effect on the equilibrium position of the reaction?

asked Jan 22 in Chemical equilibrium by JacquettaFor (470 points)

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1 answer 36 views

An industrial process involves the reaction of nitrogen gas and hydrogen gas to produce ammonia gas, in the presence of a catalyst. If the equilibrium constant for this reaction at a certain temperature is 6.2 × 10^-2 and the initial concentrations of nitrogen and hydrogen gases are 1.2 M and 0.8 M respectively, what would be the equilibrium concentrations of the reactants and products if the catalyst increases the rate of the forward reaction by a factor of 4?

asked Jan 22 in Chemical equilibrium by CarissaGibbs (490 points)

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1 answer 6 views

Ammonia and hydrochloric acid react to form ammonium chloride according to the equation: NH3(g) + HCl(g) ⇌ NH4Cl(s). If a student were to add 0.1 moles of NH4Cl to the mixture at equilibrium and the volume of the container is constant, what will be the new concentration of NH3(g) and HCl(g) in the mixture?

asked Jan 22 in Chemical equilibrium by CurtMinnis56 (570 points)

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1 answer 54 views

A student wishes to prepare a buffer solution by adding 0.20 moles of acetic acid (Ka = 1.8 x 10^-5) and 0.20 moles of sodium acetate in 1 liter of solution. The student adds 0.05 moles of hydrochloric acid (HCl) to the solution. Calculate the effect of adding the buffer on the equilibrium position of the acid-base reaction and determine the new pH of the solution.

asked Jan 22 in Chemical equilibrium by AlbertoRodge (490 points)

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1 answer 38 views

A student wants to know how the equilibrium position of a weak acid such as acetic acid would be affected if they add more acetate ion. If the initial concentration of acetic acid is 0.1 M and initial concentration of acetate ion is 0.05 M. What will be the new concentration of acetate ion necessary to increase the pH of the solution by 0.5 units?

asked Jan 22 in Chemical equilibrium by AsaHerman542 (510 points)

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1 answer 45 views

A student wants to know how changing the volume affects the position of the equilibrium for the reaction N2(g) + 3H2(g) ⇌ 2NH3(g). If the reaction is initially at equilibrium in a 2 L container at 400 K and then the volume is decreased to 1 L, what will be the new concentrations of each gas at equilibrium? (Assume that the pressure remains constant and that the reaction follows the ideal gas law.)

asked Jan 22 in Chemical equilibrium by GroverSisco (450 points)

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1 answer 45 views

A student wants to investigate the effect of volume change on the equilibrium position of the reaction 2SO2(g) + O2(g) ⇄ 2SO3(g). The initial equilibrium concentration of SO3 is 0.1 M at a constant temperature. The volume is reduced by half at equilibrium. Calculate the new equilibrium concentrations of SO2, O2 and SO3 assuming the equilibrium constant (Kc) of the reaction remains constant.

asked Jan 22 in Chemical equilibrium by LurleneWest0 (350 points)

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1 answer 43 views

A student wants to determine the ionization constant of a weak acid. They use the initial concentration and the pH of the solution at a given temperature to calculate the ionization constant. Given that the temperature of the solution is changed by 10°C, how will this affect the ionization constant of the weak acid? Calculate the new ionization constant at the new temperature assuming that no additional acid or base is added to the solution.

asked Jan 22 in Chemical equilibrium by XLOAlva5964 (450 points)

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1 answer 98 views

A student prepares a solution of 0.1 M acetic acid and 0.1 M sodium acetate in a 500 mL volumetric flask. If the pH of the solution is initially 4.7, what will be the new pH of the solution after adding 0.01 mol of hydrochloric acid?

asked Jan 22 in Chemical equilibrium by HalinaIvy91 (470 points)

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1 answer 50 views

A student prepared a 0.2 M solution of sodium acetate and the equilibrium reaction for sodium acetate is CH3COO- + H2O ⇌ CH3COOH + OH-. The initial pH of the solution is 9. Calculate the new pH of the solution when 0.1 mol of NaOH is added to it.

asked Jan 22 in Chemical equilibrium by ElenaSchoenh (490 points)

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1 answer 47 views

A student mixed 0.1 M solution of NH3 and 0.1 M solution of NH4Cl to form a buffer solution of NH3/NH4+. If the initial pH of the solution is 9.25, what will be the final pH of the solution when 0.01 moles of HCl is added? (Assume the volume of the solution is constant).

asked Jan 22 in Chemical equilibrium by AlexandraCru (510 points)

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1 answer 9 views

A student has a solution of AlF3 with a concentration of [AlF3] = 0.015 M, which is in equilibrium according to the equation: AlF3 (s) ⇌ Al3+ (aq) + 3 F- (aq). Calculate the new equilibrium concentration of F- ions if 0.001 mol of NaF is added to the solution initially at equilibrium. (Ksp of AlF3 = 2.0 x 10^-23, NaF is a common ion with F-)

asked Jan 22 in Chemical equilibrium by RolandCoble3 (490 points)

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1 answer 86 views

A student has a solution of acetic acid (CH3COOH) with a concentration of 0.1 M and wants to calculate the effect of adding sodium acetate (NaCH3COO) with a concentration of 0.05 M on the equilibrium position of the reaction CH3COOH + H2O ↔ CH3COO- + H3O+. Calculate the new equilibrium concentrations of all species and explain the effect of the added common ion on the equilibrium position.

asked Jan 22 in Chemical equilibrium by DesireeRoeme (450 points)

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1 answer 40 views

A student adds 0.1 M HCl to a solution containing 0.05 M NaOH. Calculate the effect on the equilibrium position of the system after adding a buffer solution consisting of 0.1 M CH3COOH and 0.1 M CH3COONa. Assume the dissociation constant (Ka) of CH3COOH is 1.8x10^-5.

asked Jan 22 in Chemical equilibrium by IMBDominik40 (430 points)

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1 answer 45 views

A solution of nitrogen dioxide, NO2 gas, at a pressure of 2.50 atm and temperature of 300 K, reacts with oxygen gas, O2, to form nitrogen oxide, NO, and dioxide, NO2. Write the balanced chemical equation for the reaction and determine the equilibrium concentrations of all species if the value of the equilibrium constant, Kc, at 300 K is 4.0 x 10^-4.

asked Jan 22 in Chemical equilibrium by GloriaTerpst (370 points)

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1 answer 7 views

A solution containing 0.5 M of iron(III) ions and 0.5 M of thiocyanate ions is allowed to reach equilibrium. If the equilibrium constant of the formation of the FeSCN2+ complex ion is 3.0 x 10^3, calculate the concentration of FeSCN2+ complex ion at equilibrium when the initial concentration of thiocyanate ions is doubled.

asked Jan 22 in Chemical equilibrium by Mitch41O7315 (390 points)

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1 answer 67 views

A solution containing 0.1 M acetic acid and 0.1 M sodium acetate has a pH of 4.5. If 0.02 moles of hydrochloric acid is added to the solution, what will be the pH of the solution after equilibrium is reached? (Given pKa of acetic acid = 4.76)

asked Jan 22 in Chemical equilibrium by MathewGqg478 (310 points)

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1 answer 42 views

A sealed vessel contains a mixture of nitrogen dioxide and dinitrogen tetraoxide gases in equilibrium. If the volume of the container is increased, would the equilibrium shift towards more or less NO2? Calculate the new equilibrium constant at the new volume assuming the pressure and temperature remain constant.

asked Jan 22 in Chemical equilibrium by LTSZelma4294 (470 points)

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