6. Consider the following equilibrium: The equilibrium mixture is separated into

Question

6. Consider the following equilibrium: The equilibrium mixture is separated into 2 tubes. 1 mL of 1.0M H2C204 is added to tube 1 and 1 ml of 1.0M K2C20s is added to tube 2. Precipitates form in both tubes. what is the direction of the shift when (circle left or right) ·HCO, is ii. K2C204 is added a. left right eft right Support your choice with a 1 sentence explanation: b. Which of the following results (circle one) Hint: H2C20s is a weak acid and K C20, is a soluble salt: a. More precipitate is formed in tube 1 than in tube 2 b. More precipitate is formed in tube 2 than in tube 1 c. Both tubes will have the same amount of precipitate Support your choice with a 1 sentence explanation:

Explanation / Answer

H2C2O4 is an acid compound, it will not ionize compleatly in water where as K2C2O4 is an inorganic salt, ionizes 100% in water. So K2C2O4 produce C2O4-2 ions in waer and shift the equilibrium to right side.

1.

When HC2O4 added to the formation CaC2O4 is less, the equilibriu shift to reagent side, lefft side

When K2C2O4 added to the formation CaC2O4 is more, the equilibriu shift to product side, right side.

H2C2O4 is an acid compound, it will not ionize compleatly in water and in acidid condition, CaC2O4 solubilises in water, so left side products will be more.

where as K2C2O4 is an inorganic salt, ionizes 100% in water. So K2C2O4 produce C2O4-2 ions in waer and shift the equilibrium to right side.

2.

ans b. more precipitate formed in test tube 2. because adding the K2C2O4 drives the equiliibrium to right side, and more amount of CaC2O4 formed. And it is less soluble in water so it precipitate out.

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