You asked: What is the relationship between Q and KSP?

If Q = Ksp, a precipitate will form. If Q > Ksp, a precipitate will form. Note that precipitation may not happen immediately if Q is equal to or greater than Ksp. A solution could be supersaturated for some time until precipitation occurs.

What will happen to a solution where Q Ksp?

If more solid as added to an unsaturated solution, it dissolves until the solution is saturated (at which point there is solid in equilibrium with the solvated ions). … If Q < Ksp, the solution is unsaturated and no precipitation will occur.

Why does a precipitate form when q is greater than Ksp?

Likewise, when substituted into the equilibrium expression, a value larger than K sp results. Thus, when Q is greater than K sp results in precipitation. If Q is larger than K, then the reaction will shift to the left to establish equilibrium. Thus, BaSO 4 (s), a precipitate, forms.

What is the difference between the ion product Q and the solubility product Ksp?

The solubility product (Ksp) is used to calculate equilibrium concentrations of the ions in solution, whereas the ion product (Q) describes concentrations that are not necessarily at equilibrium.

What is Q in Ksp?

The reaction quotient, Q, can be used to determine whether a precipitate will form with a given concentration of ions. … If Q < Ksp, no precipitate will form. If Q = Ksp, a precipitate will form. If Q > Ksp, a precipitate will form.

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How do you calculate Q?

We can calculate Q by writing out the equation using the balanced reaction and then using the given concentrations. If we compare Q to K, we can see that Q > K Q > K Q>KQ, is greater than, K.

What is KSP formula?

In general, MaXb(s) <=> aM+b(aq) + bXa(aq) is expressed as Ksp = [M+b]a[Xa]b. These expressions are called solubility product constant expressions because they involve the product of the equilibrium concentrations of the constituent ions, each raised to the power corresponding to the number of ions in the formula.

What if Q is less than K?

If Q<K, then the reaction favors the products. The ratio of products to reactants is less than that for the system at equilibrium—the concentration or the pressure of the reactants is greater than the concentration or pressure of the products.

Does a higher Ksp precipitate first?

When two anions form slightly soluble compounds with the same cation, or when two cations form slightly soluble compounds with the same anion, the less soluble compound (usually, the compound with the smaller Ksp) generally precipitates first when we add a precipitating agent to a solution containing both anions (or …

What happens when Q K?

Q can be used to determine which direction a reaction will shift to reach equilibrium. If K > Q, a reaction will proceed forward, converting reactants into products. If K < Q, the reaction will proceed in the reverse direction, converting products into reactants. If Q = K then the system is already at equilibrium.

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