The acid dissociation constant (Ka) for carbonic acid (H₂CO₃) dissociating into hydrogen ions (H⁺) and bicarbonate ions (HCO₃⁻) is a measure of the strength of the acid in solution. The dissociation reaction can be represented as: H₂CO₃ (aq) ⇌ H⁺ (aq) + HCO₃⁻ (aq). The value of Ka for this process is approximately 4.3 x 10⁻⁷ at 25°C, indicating that H₂CO₃ is a weak acid.
HCN(aq) ==> H^+(aq) + CN^-(aq)Ka = [H+][CN-]/[HCN] and the value can be looked up in a book or on line.
The equilibrium constant ( K_a ) for the dissociation of carbonic acid (H₂CO₃) into hydrogen ions (H⁺) and bicarbonate ions (HCO₃⁻) can be represented by the equation: [ H_2CO_3 (aq) \rightleftharpoons H^+ (aq) + HCO_3^- (aq) ] The value of ( K_a ) for this reaction at 25°C is approximately ( 4.3 \times 10^{-7} ). This indicates that carbonic acid is a weak acid, as it does not completely dissociate in solution.
ka=[H+][NO2_]/[HNO2]
The acid dissociation constant (Ka) for the reaction of boric acid (H3BO3) in water can be expressed as: [ H3BO3(aq) \rightleftharpoons H^+(aq) + H2BO3^-(aq) ] The Ka value represents the equilibrium constant for this reaction, indicating the extent to which boric acid donates protons to form hydronium ions (H+) and the borate ion (H2BO3^-). For boric acid, this Ka is relatively small, reflecting its weak acidic nature compared to stronger acids.
The acid dissociation constant (Ka) for the dissociation of nitrous acid (HNO2) into hydrogen ions (H⁺) and nitrite ions (NO2⁻) can be expressed with the equation: [ K_a = \frac{[H^+][NO_2^-]}{[HNO_2]} ] This equilibrium constant quantifies the strength of HNO2 as an acid; a larger Ka value indicates a stronger acid, meaning it dissociates more completely in solution. For HNO2, the Ka is approximately 4.5 × 10⁻⁴ at 25°C, indicating it is a weak acid.
HCN(aq) ==> H^+(aq) + CN^-(aq)Ka = [H+][CN-]/[HCN] and the value can be looked up in a book or on line.
3.4 * 10^-8
ka=[H+][NO2_]/[HNO2]
Ka= [H+] [H2BO3-] / [h3BO3] (Apex)
ka=[H+][CN-]/[HCN]
6.6 x 10-9
Ka= [h+][HCO3-]/[H2CO3]
The acid dissociation constant (Ka) for the dissociation of nitrous acid (HNO2) into hydrogen ions (H⁺) and nitrite ions (NO2⁻) can be expressed with the equation: [ K_a = \frac{[H^+][NO_2^-]}{[HNO_2]} ] This equilibrium constant quantifies the strength of HNO2 as an acid; a larger Ka value indicates a stronger acid, meaning it dissociates more completely in solution. For HNO2, the Ka is approximately 4.5 × 10⁻⁴ at 25°C, indicating it is a weak acid.
The equilibrium constant expression for the reaction you provided would be ( K_a = \frac{[H^+][H_2BO_3^-]}{[H_3BO_3]} ). However, the specific value of ( K_a ) for this reaction would depend on the concentrations of the species involved in the particular experimental conditions.
The Ka for the dissociation of HNO2 is 4.5 x 10^-4. This value represents the equilibrium constant for the reaction of HNO2 dissociating into H+ and NO2-.
not sure
Ka= [H+][NO2-] [HNO2]