NeilynAcosta Name 1.Determine the [H3O*] in a 0.265 M HCIO solution. The Ka of HCIO is 2.9 × 10-8. 2.9X10-8- X • X 0.265-X x2=7.685 x10-9 HCUO(aq)+ HaD ()→ CIO lag)+ H2D * aq) -> I 0.2165 %3D [HC I0] CI -X x+ X+ X= 8.1 66 x10-5 E0-265x| . 2l05-x H30+] = 6.16lox1D-6 %3D 2.Determine pH and percent ionization for a 0.015M acetic acid solution at 25°C. The Ka for acetic acid solution is Ka= 1.8 X10-5 3. At 2000 °C the equilibrium constant for the reaction below is Kc= 2.4x10³ . If the initial concentration of NO is 0.500 M, what are the equilibrium concentrations of each substance? 2 NO (g) = N2 (g) + 02 (g) 4. At a certain temperature the equilibrium constant, Kc, equals 0.11 for the reaction: 2 ICI(g) = 12(g) + Cl2(g). What is the equilibrium concentration of ICl if mol of I2 and 0. 45 mol of Cl2 are
NeilynAcosta Name 1.Determine the [H3O*] in a 0.265 M HCIO solution. The Ka of HCIO is 2.9 × 10-8. 2.9X10-8- X • X 0.265-X x2=7.685 x10-9 HCUO(aq)+ HaD ()→ CIO lag)+ H2D * aq) -> I 0.2165 %3D [HC I0] CI -X x+ X+ X= 8.1 66 x10-5 E0-265x| . 2l05-x H30+] = 6.16lox1D-6 %3D 2.Determine pH and percent ionization for a 0.015M acetic acid solution at 25°C. The Ka for acetic acid solution is Ka= 1.8 X10-5 3. At 2000 °C the equilibrium constant for the reaction below is Kc= 2.4x10³ . If the initial concentration of NO is 0.500 M, what are the equilibrium concentrations of each substance? 2 NO (g) = N2 (g) + 02 (g) 4. At a certain temperature the equilibrium constant, Kc, equals 0.11 for the reaction: 2 ICI(g) = 12(g) + Cl2(g). What is the equilibrium concentration of ICl if mol of I2 and 0. 45 mol of Cl2 are
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![NeilynAcosta
Name
1.Determine the [H3O*] in a 0.265 M HCIO solution. The Ka of HCIO is 2.9 × 10-8.
2.9X10-8- X • X
0.265-X
x2=7.685 x10-9
HCUO(aq)+ HaD ()→ CIO lag)+ H2D * aq)
->
I 0.2165
%3D
[HC I0]
CI -X
x+
X+
X= 8.1 66 x10-5
E0-265x|
. 2l05-x
H30+] = 6.16lox1D-6
%3D
2.Determine pH and percent ionization for a 0.015M acetic acid solution at 25°C. The Ka
for acetic acid solution is Ka= 1.8 X10-5
3. At 2000 °C the equilibrium constant for the reaction below is Kc= 2.4x10³ . If the initial
concentration of NO is 0.500 M, what are the equilibrium concentrations of each
substance?
2 NO (g) = N2 (g) + 02 (g)
4. At a certain temperature the equilibrium constant, Kc, equals 0.11 for the reaction:
2 ICI(g) = 12(g) + Cl2(g).
What is the equilibrium concentration of ICl if
mol of I2 and 0. 45 mol of Cl2 are](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F57c52580-fa5a-4aad-906a-3a46491efd67%2F6775e61b-2fa7-4322-b20f-09a79b794082%2Fodmqakj.jpeg&w=3840&q=75)
Transcribed Image Text:NeilynAcosta
Name
1.Determine the [H3O*] in a 0.265 M HCIO solution. The Ka of HCIO is 2.9 × 10-8.
2.9X10-8- X • X
0.265-X
x2=7.685 x10-9
HCUO(aq)+ HaD ()→ CIO lag)+ H2D * aq)
->
I 0.2165
%3D
[HC I0]
CI -X
x+
X+
X= 8.1 66 x10-5
E0-265x|
. 2l05-x
H30+] = 6.16lox1D-6
%3D
2.Determine pH and percent ionization for a 0.015M acetic acid solution at 25°C. The Ka
for acetic acid solution is Ka= 1.8 X10-5
3. At 2000 °C the equilibrium constant for the reaction below is Kc= 2.4x10³ . If the initial
concentration of NO is 0.500 M, what are the equilibrium concentrations of each
substance?
2 NO (g) = N2 (g) + 02 (g)
4. At a certain temperature the equilibrium constant, Kc, equals 0.11 for the reaction:
2 ICI(g) = 12(g) + Cl2(g).
What is the equilibrium concentration of ICl if
mol of I2 and 0. 45 mol of Cl2 are
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