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Verified answer
Ka= [H+][NO2-]
[HNO2]
Wiki User
∙ 11y ago
Natalie Steger
Colin Evans
What is Ka for HNO2(aq) H (aq) NO2-(aq)?
ka=[H+][NO2_]/[HNO2]
What is Ka for H3BO3(aq) H (aq) H2BO3-(aq)?
not sure
What is Ka for HCN aq H aq CN aq?
ka=[H+][CN-]/[HCN]
What is Ka for H3BO3(aq) = H+(aq)+H2BO3 -(aq)?
Ka= [H+] [H2BO3-] / [h3BO3] (Apex)
What is Ka for H2CO3 aq H aq HCO3 aq?
Ka= [h+][HCO3-]/[H2CO3]
What is Ka for HNO2(aq) NO2 (aq)?
ka=[H+][NO2_]/[HNO2]
What is Ka for HNO2(aq) H (aq) NO2-(aq)?
ka=[H+][NO2_]/[HNO2]
What is Ka for H3BO3(aq) H (aq) H2BO3-(aq)?
not sure
What is Ka for HCN aq H aq CN aq?
ka=[H+][CN-]/[HCN]
What is Ka for H3BO3(aq) = H+(aq)+H2BO3 -(aq)?
Ka= [H+] [H2BO3-] / [h3BO3] (Apex)
What is Ka for H2CO3 aq H aq HCO3 aq?
Ka= [h+][HCO3-]/[H2CO3]
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 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
Which equation represents the total ionic equation for the reaction of HNO3 and NaOH?
The equation is:H+ + (NO3)- + Na+ + (OH)- = (NO3)- + Na+ + H2O (2 H+ OH-)
Nitrous acid has a Ka of 4.7x10-4. What is the pH of a buffer solution containing 0.15 M HNO2 and 0.20 M NO2?
Use the Henderson-Hasselbalch equation:[H+] = Ka * [HA] / [A-]where[HA] = concentration HNO2 (acid) and[A-] = concentration NO2- (base) andKa = 4.7*10-4Filling in and calculating: [H+] = Ka * [HA] / [A-] = (4.7*10-4) * (0.15) / (0.20) = 3.5*10-4 ,so :pH = -log[H+] = -log(3.5*10-4) = 3.45
What is the pH of a 0.020 M nitric acid solution?
HNO2 ==> H+ + NO2^-Ka = 4x10^-4 = [H+][NO2^-]/[HNO2] 4x10^-4 = (x)(x)/0.100 x^2 = 4x10^-5 x = 6.32x10^-3 = [H+] pH = -log 6.32x10^-3 pH = 2.2
What is the net ionic equation for the reaction of aqueous perchloric acid and aqueous potassium hydroxide?
The two will react to form salt and water HCOOH (aq)+ KOH(aq) --> HCOOK(aq) + H2O(l) In ionic form, HCOOH + K+ + OH- --> HCOO- + K+ + H2O HCOOH is weak acid so it should not be written in ionic form. K+ ions cancel out leaving HCOOH + OH- --> HCOO- + H2O (net ionic equation)
