![Reaction [H2CO3] Initia [HCO3) 4.58 x 10-3 -y 0.00458 - y TOH-1 0.00458 +y Change + y Equilibrium 0.00458 + y • K12 = 2.4 x 1](http://img.homeworklib.com/questions/613ca420-1007-11ec-b6e1-63c27d5e230b.png?x-oss-process=image/resize,w_560)
![Solution Reaction Initial Change Equilibrium (HC,01_ 0.10 U 0.10 - X (HC,02 0 + x [H,01 0 + x tx • Ka = 5.9 x 10-2 = (HC204][](http://img.homeworklib.com/questions/62e47850-1007-11ec-900d-bb9438d29edf.png?x-oss-process=image/resize,w_560)
Homework Answers
This is a quadratic equation in this two cases which are solved to get the x and y.
In case of H2CO3, 0.00458+y=0.00458 as y is very small.
So, y=Kb2
x2=(0.1-x)×5.9×10-2.
x2-5.9×10-3+5.9×10-2x. this is of the form ax2+bx+c=0
Root is x=-b
√(b2-4ac)/2a,
we get x.
Similarly, y2+0.0528y=-6.4×10-5y+3.4×10-6
y2+0.05806y-3.4×10-6=0
Solving in y we get the value given.
correct answer is highlighted in pink. how do i get the pH without it being 1.6?...
correct answer is highlighted in pink. how do i get
the pH without it being 1.6?
Equilibrium Constants The following equilibrium constants will be useful for some of the problems. Substance H2CO3 Substance HCOH HNO2 НОСІ (COOH)2 Constant K = 1.8 x 10-4 Ka = 4.5 x 10-4 KA = 3.5 x 10-8 K = 7.2 x 10-4 KA = 4.0 x 10-10 Ki = very large K = 1.2 x 10-2 Ka=2.5 x 10-9 Constant Ki = 4.2 x...
Explain the process of how to get the answer. The answer is highlighted. Ch. 18 Values...
Explain the process of how to get the answer. The
answer is highlighted.
Ch. 18 Values The following values will be useful for problems in this chapter. Acid Substance or Species HF HNO2 CH3COOH HOCI HOBr HOCN HCN H2SO4 KA = 7.2 x 10-4 Ka = 4.5 x 10-4 Ka = 1.8 x 10-5 Ka = 3.5 x 10-8 = 2.5 x 10-9 K4 = 3.5 x 10-4 Ka = 4.0 x 10-10 Kai = very large Kq2 = 1.2...
i need help with both :( 33. What is the pH of a 0.75 M Benzoic...
i need help with both :(
33. What is the pH of a 0.75 M Benzoic Acid (HC H3O2) solution? Ka for Benzoic Acid is 6.4 x 10-5 34. What is the pH of a 0.040 M Pyridine (CsH5N) solution? Kb for Pyridine is 1.7 x 10-9
I need the highlighted parts, and check if what I did is correct. Thanks! I. Equilibrium...
I need the highlighted parts,
and check if what I did is correct. Thanks!
I. Equilibrium Glacial CH3COOH Final buret reading 46 Moles acetic acid 0.0524 used (show work) Molarity of solution (show work) Initial buret reading 49 0.524 mL acetic acid used 3 mL H30 1eq 1.4125 x 10-3 pH measured 2.85 Using appropriate concentrations, complete the "I", "C", "E" table below [CH3COO- [CH:COОH] 0.524 [H:О"] Initial concentrations +1.4125x10-3 1.4125x10-3 +1.4125x10-3 1.4125x10-3 Change Equilibrium Conc Calculate the value of...
1.0 x 100 M 1.3 x 105 4.0 x 1011 M 1.6*10-10 M QUESTION 4 At...
1.0 x 100 M 1.3 x 105 4.0 x 1011 M 1.6*10-10 M QUESTION 4 At 450°C, tert-butyl alcohol decomposes into water and isobutene: (CH3)3COH(g) = (CH3)2CCH2(g) + H2O(g) A reaction vessel containing these compounds is at equilibrium. What will happen to the equilibrium If the volume of the container is reduced by 50% at constant temperature? The equilibrium constant will increase. The equilibrium constant will decrease. The reverse reaction will proceed to re-establish equilibrium. The forward reaction will proceed...
I need help with #4. "show by calculation why acetic acid (Ka = 1.8 X 10^-5), when combined with NaC2H3O3 as a buffe...
I need help with #4. "show by calculation why acetic
acid (Ka = 1.8 X 10^-5), when combined with NaC2H3O3 as a buffer,
will not produce a pH o 9.00"
1. What is the pH of a 1.0L buffer that is 0.10 M in Naz HPO4 and 0.15 M in NaH2PO4? Write the equilibrium reaction equation and corresponding Ka expression for the buffer. K for H2PO4 is 6.2 X 108 2. A 10.00 mL sample of 0.300 M NH3 is...
please show all work for part III :) all the information needed is in the pictures...
please show all work for part III :) all the information
needed is in the pictures
III. Preparing HC,HO, Solutions and Determining pH only cal. One! theoretical pH 1.0 x 10-14 (181) concentration of HC,H,O, M measured pH ya ? 3.06 1.0 x 10-2 ka: 1. 8x10°3 ixio- 3.43 1.0 x 10-3 x = CH) -1,34% 103n 3.87 1.0 x 107 PM - 04 TH11 4.30 concentration of HC,H,O, M calculated K of HC H302 based on pH data literature...
In need of help 1 – List four factors that affect the strength of an acid....
In need of help 1 – List four factors that affect the strength of an acid. All four may not apply to every acid. 2 – Calculate [OH-] for a 1.4 x 10-3 M HCl solution. 3 – Calculate the pH of an aqueous solution at 25 ̊C at is 0.34 M in phenol (Ka = 1.3 x 10-10) .4 – Calculate the concentration at which a monoprotic acid with Ka = 4.5 x 10-5 will be 2.5% ionized. (The...
need help with 42 & 44 I am trying to figure out how to make a...
need help with 42 & 44
I
am trying to figure out how to make a desired buffer
42. What volumes of 0.50 M HNO2 and 0.50 M NaNO2 must be mixed to prepare 1.00 L of a solution buffered at pH = 3.55? 43. Consider a solution that contains both C5H5N and C5H5NHNO3. Calculate the ratio (C3H5N]/[C3H5NH+] if the solution has the following pH values: a. pH = 4.50 c. pH = 5.23 l g de to b. pH...
The answer is not 2.4 x 10^-9. Here is an example on how to do these...
The answer is not 2.4 x 10^-9.
Here is an example on how to do these type of problems.
Use the References to access important values if needed for this question. When 22.0 mL of a 5.45*10-4 M ammonium sulfide solution is combined with 22.0 mL of a 1.76*10* Miron(II) nitrate solution does a precipitate form? yes (yes or no) For these conditions the Reaction Quotient, Q, is equal to Use the References to access important values if needed for...
correct answer is highlighted in pink. how do i get
the pH without it being 1.6?
Equilibrium Constants The following equilibrium constants will be useful for some of the problems. Substance H2CO3 Substance HCOH HNO2 НОСІ (COOH)2 Constant K = 1.8 x 10-4 Ka = 4.5 x 10-4 KA = 3.5 x 10-8 K = 7.2 x 10-4 KA = 4.0 x 10-10 Ki = very large K = 1.2 x 10-2 Ka=2.5 x 10-9 Constant Ki = 4.2 x...
Explain the process of how to get the answer. The
answer is highlighted.
Ch. 18 Values The following values will be useful for problems in this chapter. Acid Substance or Species HF HNO2 CH3COOH HOCI HOBr HOCN HCN H2SO4 KA = 7.2 x 10-4 Ka = 4.5 x 10-4 Ka = 1.8 x 10-5 Ka = 3.5 x 10-8 = 2.5 x 10-9 K4 = 3.5 x 10-4 Ka = 4.0 x 10-10 Kai = very large Kq2 = 1.2...
i need help with both :(
33. What is the pH of a 0.75 M Benzoic Acid (HC H3O2) solution? Ka for Benzoic Acid is 6.4 x 10-5 34. What is the pH of a 0.040 M Pyridine (CsH5N) solution? Kb for Pyridine is 1.7 x 10-9
I need the highlighted parts,
and check if what I did is correct. Thanks!
I. Equilibrium Glacial CH3COOH Final buret reading 46 Moles acetic acid 0.0524 used (show work) Molarity of solution (show work) Initial buret reading 49 0.524 mL acetic acid used 3 mL H30 1eq 1.4125 x 10-3 pH measured 2.85 Using appropriate concentrations, complete the "I", "C", "E" table below [CH3COO- [CH:COОH] 0.524 [H:О"] Initial concentrations +1.4125x10-3 1.4125x10-3 +1.4125x10-3 1.4125x10-3 Change Equilibrium Conc Calculate the value of...
1.0 x 100 M 1.3 x 105 4.0 x 1011 M 1.6*10-10 M QUESTION 4 At 450°C, tert-butyl alcohol decomposes into water and isobutene: (CH3)3COH(g) = (CH3)2CCH2(g) + H2O(g) A reaction vessel containing these compounds is at equilibrium. What will happen to the equilibrium If the volume of the container is reduced by 50% at constant temperature? The equilibrium constant will increase. The equilibrium constant will decrease. The reverse reaction will proceed to re-establish equilibrium. The forward reaction will proceed...
I need help with #4. "show by calculation why acetic
acid (Ka = 1.8 X 10^-5), when combined with NaC2H3O3 as a buffer,
will not produce a pH o 9.00"
1. What is the pH of a 1.0L buffer that is 0.10 M in Naz HPO4 and 0.15 M in NaH2PO4? Write the equilibrium reaction equation and corresponding Ka expression for the buffer. K for H2PO4 is 6.2 X 108 2. A 10.00 mL sample of 0.300 M NH3 is...
please show all work for part III :) all the information
needed is in the pictures
III. Preparing HC,HO, Solutions and Determining pH only cal. One! theoretical pH 1.0 x 10-14 (181) concentration of HC,H,O, M measured pH ya ? 3.06 1.0 x 10-2 ka: 1. 8x10°3 ixio- 3.43 1.0 x 10-3 x = CH) -1,34% 103n 3.87 1.0 x 107 PM - 04 TH11 4.30 concentration of HC,H,O, M calculated K of HC H302 based on pH data literature...
need help with 42 & 44
I
am trying to figure out how to make a desired buffer
42. What volumes of 0.50 M HNO2 and 0.50 M NaNO2 must be mixed to prepare 1.00 L of a solution buffered at pH = 3.55? 43. Consider a solution that contains both C5H5N and C5H5NHNO3. Calculate the ratio (C3H5N]/[C3H5NH+] if the solution has the following pH values: a. pH = 4.50 c. pH = 5.23 l g de to b. pH...
The answer is not 2.4 x 10^-9.
Here is an example on how to do these type of problems.
Use the References to access important values if needed for this question. When 22.0 mL of a 5.45*10-4 M ammonium sulfide solution is combined with 22.0 mL of a 1.76*10* Miron(II) nitrate solution does a precipitate form? yes (yes or no) For these conditions the Reaction Quotient, Q, is equal to Use the References to access important values if needed for...
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