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At a certain temperature a 0.16 m solution of hcn has a pH of 4.29 what is the ka of hcn at this temperature?
A pH of 4.29 corresponds to a hydrogen ion concentration of 10-4.29, which equals 10-5 X 10+0.71, since 0.71 - 5 = -4.29. 10+0.71 = 5.1, to the justified number of significant digits. By definition, Ka = [H+]X[CN-]/[HCN], and in the absence of other sources of cyanide anions, [H+] = [CN-]. Within the number of significant digits given, [HCN] = 0.16, and Ka then = (5.1 X 10-5)2/0.16 = 1.6 X 10-8.
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 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) NO2 (aq)?
ka=[H+][NO2_]/[HNO2]
What is the Ka for aspirin with a pka of 3.48?
All you need to do to get Ka is to take the antilog of the pKa.
What is Ka for HCN aq H aq CN aq?
ka=[H+][CN-]/[HCN]
At a certain temperature a 0.16 m solution of hcn has a pH of 4.29 what is the ka of hcn at this temperature?
A pH of 4.29 corresponds to a hydrogen ion concentration of 10-4.29, which equals 10-5 X 10+0.71, since 0.71 - 5 = -4.29. 10+0.71 = 5.1, to the justified number of significant digits. By definition, Ka = [H+]X[CN-]/[HCN], and in the absence of other sources of cyanide anions, [H+] = [CN-]. Within the number of significant digits given, [HCN] = 0.16, and Ka then = (5.1 X 10-5)2/0.16 = 1.6 X 10-8.
What is 1 plus 1-1x1-1 plus 1x1?
tanga ka pam
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Agar 5 plus 4 equals 919 ho saktay hain to 7 plus 2 ka kya answer ho ga?
959
What is the acid dissociation constant for an acid at equilibrium HX ----- H (spuare Plus) plus x -?
The acid dissociation constant, Ka, is a measure of how well an acid donates a proton in a chemical reaction. For the reaction HX ⇌ H+ + X-, the expression for Ka is [H+][X-]/[HX]. The value of Ka indicates the strength of the acid - higher Ka values indicate stronger acids.
Calculate the pH of a 0.028 m NACN solution Ka 4.9 x 10 -10. the answer is 10.88 please help?
This is a weak base problem. Assume F = 0.028M Ka = 4.9 10^-10 Kb = Kw / Ka Kw - 10^-14 therefor pKw=14 x = [OH-] Kw / Ka = Kb = x^2 / (F-x) solve for "x" by use of quadratic formula to get the [OH-] pOH = -log [OH-] then plug pOH into the pH equation pH =pKw - pOH
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 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.
1 plus 3 plus 5 plus 7 plus 9 plus 11 plus 13 plus 15 plus 17 plus 19 ka total agar 100 banta hai to se 5 no. hai jinka total 50 banta hai?
kyoki agar odd no. ko odd bar plus kare to odd hi aayega
Consider the reaction nh2oh aq plus h2ol nh3oh plus aq plus h3o plus aq if ka equals 1.5 x 10-6 for nh3oh plus what is kb for nh2oh kw equals 1.0 x 10-14 at this temperature?
6.6 x 10-9
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A Birdie ka ka ka ka like a birdie...birdie
