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What is Ka for HCN aq H aq CN aq?
ka=[H+][CN-]/[HCN]
What is Ka for HNO2(aq) NO2 (aq)?
ka=[H+][NO2_]/[HNO2]
What is Ka for H3BO3(aq) = H+(aq)+H2BO3 -(aq)?
Ka= [H+] [H2BO3-] / [h3BO3] (Apex)
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 aq HCO3 aq?
Ka= [h+][HCO3-]/[H2CO3]
What is Ka for H3BO3(aq) H (aq) H2BO3-(aq)?
not sure
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 Ka for HNO2 aq H aq NO2-aq?
Ka= [H+][NO2-] [HNO2]
What is Ka for H3PO4(aq) H (aq) H2PO4-(aq)?
Since H3PO4 has 3 ionizable hydrogens, it will have three Ka values. Approximate values areKa1 = 7x10^-3; Ka2 = 6x10^-8 and Ka3 = 4.5x10^-13
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 H3BO3aq H aq H2BO3-aq?
The dissociation of boric acid (H₃BO₃) in aqueous solution involves the formation of the borate ion (H₂BO₃⁻) and a proton (H⁺). The acid dissociation constant (Ka) for this reaction is typically around 5.8 x 10⁻¹⁰ at 25°C. This indicates that boric acid is a weak acid, as it does not completely dissociate in water.
What is Ka for H2CO3aq H aq HCO3aq?
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.
