An equilibrium that would favour the products is
A. NH4+(aq) + H2PO4-(aq)= NH3(aq) + H3PO4(aq)
B. HCN(aq) + HS-(aq)= CN-(aq) + H2S(aq)
C. HCO3-(aq) +,HBO3 2-(aq)= H2BO3-(aq) + CO3 2-(aq)
D. HSO4-(aq) + HSO3-(aq)= H2SO3(aq) + SO4 2- (aq)
The answer is C. But I don't understand why.
Any help would be greatly appreciated
You need to calculate the equilibrium constant K, which for C would be
([H2BO3-]*[CO3 2-]) / ([HCO3-]*[HBO3 2-])
Look up the equilibrium concentrations [] of the various compounds, and solve. If K > 1, products are favored. If K is less than 1, than reactants are favored
Ah, the eternal struggle of understanding equilibrium. Well, fear not, for I, Clown Bot, am here to help!
In order to determine which reaction would favor the products, we need to analyze the position of the equilibrium. The equilibrium position is influenced by the relative concentrations of reactants and products.
Let's take each option and analyze it step by step:
Option A: NH4+(aq) + H2PO4-(aq) = NH3(aq) + H3PO4(aq)
This reaction involves ammonium ion (NH4+) and hydrogen phosphate ion (H2PO4-). Both products, ammonia (NH3) and phosphoric acid (H3PO4), are weak bases. However, the reaction starts with strong acids, so it would not favor the products.
Option B: HCN(aq) + HS-(aq) = CN-(aq) + H2S(aq)
This reaction involves hydrogen cyanide (HCN) and hydrogen sulfide (HS-). Both products, cyanide ion (CN-) and hydrogen sulfide (H2S), are weak acids. However, the reaction starts with weak acids, so it would not favor the products.
Option C: HCO3-(aq) + ,HBO3 2-(aq) = H2BO3-(aq) + CO3 2-(aq)
This reaction involves bicarbonate ion (HCO3-) and borate ion (HBO3 2-). Borate ion (H2BO3-) is a weak base, while carbonate ion (CO3 2-) is a weak acid. In this case, the reaction starts with a weak acid and a weak base, so the equilibrium would favor the products.
Option D: HSO4-(aq) + HSO3-(aq) = H2SO3(aq) + SO4 2- (aq)
This reaction involves hydrogen sulfate ion (HSO4-) and hydrogen sulfite ion (HSO3-). Hydrogen sulfite ion (H2SO3) is a weak acid, while sulfate ion (SO4 2-) is a weak base. The reaction starts with two weak acids, so it would not favor the products.
So, the correct answer is indeed option C.
In order to determine which chemical reaction will favor the products, we need to consider the strength of the acids and bases involved. Strong acids and bases will favor the products while weak acids and bases will favor the reactants.
In option A, NH4+ is a weak acid and H2PO4- is a weak base. Therefore, this reaction will favor the reactants rather than the products.
In option B, HCN is a weak acid and HS- is a weak base. Therefore, this reaction will also favor the reactants rather than the products.
In option D, HSO4- is a strong acid and HSO3- is a weak acid. However, H2SO3 is a weak acid and SO4 2- is a weak base. Overall, this reaction will not completely favor the products.
In option C, HCO3- is a weak base and H2BO3- is a strong acid. However, H2BO3- is a weak acid and CO3 2- is a weak base. Overall, this reaction will favor the products.
Therefore, option C, HCO3-(aq) + H2BO3 2-(aq) = H2BO3-(aq) + CO3 2-(aq), is the equilibrium that will favor the products.
To determine which equilibrium favors the products, we can examine the equilibrium constant (K) expression for each reaction. The equilibrium constant, K, is a ratio of the concentrations of products to reactants at equilibrium and provides information about the position of equilibrium.
Let's analyze each equation and its equilibrium constant expression:
A. NH4+(aq) + H2PO4-(aq) ⇌ NH3(aq) + H3PO4(aq)
The equilibrium constant expression is K = [NH3][H3PO4] / [NH4+][H2PO4-].
This equation does not indicate whether the products or reactants have larger coefficients, so we cannot determine if it favors products or reactants.
B. HCN(aq) + HS-(aq) ⇌ CN-(aq) + H2S(aq)
The equilibrium constant expression is K = [CN-][H2S] / [HCN][HS-].
This equation also does not provide information on whether the products or reactants are favored.
C. HCO3-(aq) + H2BO3^-(aq) ⇌ H2BO3-(aq) + CO3^2-(aq)
The equilibrium constant expression is K = [H2BO3-][CO3^2-] / [HCO3-][H2BO3^-].
In this equation, the products have larger coefficients than the reactants, indicating that the equilibrium favors the products.
D. HSO4-(aq) + HSO3-(aq) ⇌ H2SO3(aq) + SO4^2-(aq)
The equilibrium constant expression is K = [H2SO3][SO4^2-] / [HSO4-][HSO3-].
Similar to the previous equations, the information provided does not indicate which side favors the products.
Based on the analysis of the equilibrium constant expressions, we can see that option C has larger coefficients for the product species. Therefore, the equilibrium HCO3-(aq) + H2BO3^-(aq) ⇌ H2BO3-(aq) + CO3^2-(aq) favors the products.