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What is Ka for HNO2(aq) NO2 (aq)?
ka=[H+][NO2_]/[HNO2]
What is ka for HNO2(aq) H plus (aq) plus NO2-(aq)?
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.
What is Ka for HCN(aq) H plus (aq) plus CN and ndash(aq)?
HCN(aq) ==> H^+(aq) + CN^-(aq)Ka = [H+][CN-]/[HCN] and the value can be looked up in a book or on line.
What is Ka for H2CO3(aq)H plus (aq) plus HCO3-(aq))?
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.
What is a Ka for H3BO3(aq) H(aq) plus H2BO3(aq)?
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.
What is Ka for HNO2(aq) NO2 (aq)?
ka=[H+][NO2_]/[HNO2]
What is Ka for HNO2(aq) H (aq) NO2-(aq)?
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-.
What is Ka for HNO2 aq H aq NO2-aq?
Ka= [H+][NO2-] [HNO2]
What is ka for HNO2(aq) H plus (aq) plus NO2-(aq)?
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.
What is Ka for HCN(aq) H plus (aq) plus CN and ndash(aq)?
HCN(aq) ==> H^+(aq) + CN^-(aq)Ka = [H+][CN-]/[HCN] and the value can be looked up in a book or on line.
How do you write nitrous acid in solution?
Nitrous acid in solution can be written as HNO2(aq).
What is the chemical Formula of barium nitrate in water?
Equilibrium:NO2- (aq) + H2O HNO2 (aq) + OH- (aq)
What is the compound HNO2(aq)?
Hydrogen nitrite acid
Consider the reaction hocl aq plus H2O l ocl-aq plus h3o plus aq if kb equals 2.9 x 10-7 for ocl-what is ka for hocl?
3.4 * 10^-8
What is Ka for H2CO3(aq)H plus (aq) plus HCO3-(aq))?
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.
What is the compound HNO2 aq?
It is able to (completely) donate its protons (H+) to water when in dilute solution (protolysis). This is what, according to Bronsted-Lowry, makes it a (strong) acid.HNO3 + H2O --> H3O+ + NO3-
What is Ka for H3BO3(aq) = H+(aq)+H2BO3 -(aq)?
Ka= [H+] [H2BO3-] / [h3BO3] (Apex)
