Can you please show math, formulas and explain. 1. If the pH of a solution is...
Can you please show math, formulas and explain.
1. If the pH of a solution is 7.5, what is the pOH? pH = - log[H+] [H+][OH-] = 1.0 x 10-14 M2
2. Given the Ka values for two acids, determine the pKas and which is a stronger acid. Ka1 = 1.38 × 10–7 Ka2 = 1.70 × 10–4
3. The pH of a sample of blood is 7.4, while gastric juice is pH 2.4. The blood sample has:
A) one hundred thousand times lower [H+] than the gastric juice.
B) 5000 times lower [H+] than the gastric juice.
C) 0.189 times the [H+] as the gastric juice.
D) 5 times lower [H+] than the gastric juice.
E) 5.29 times lower [H+] than the gastric juice.
Answer is A, can you explain please
4. Calculate the pKa of formic acid to determine the buffering range, given a concentration of formic acid of 0.050 M and the concentration of formate is 0.158 M, the pH of the solution is 4.25. Use the pKa to determine the buffering range. [ A- ] pH = pKa + log(A-/HA)
Homework Answers
Add Answer to:
Can you please show math, formulas and explain.
1. If the pH of a solution is...
1. 1x10^-9 moles of strong acid HCl are added to of water (total volume is 1L)....
1. 1x10^-9 moles of strong acid HCl are added to of water (total volume is 1L). the pH of the resulting solution is... a)9 b)8 c)7 d)5 e)2 I got 9 but got the answer incorrect, so i would like to know how to solve this properly and what is the final answer. 2. the pKa of acetic acid is 4.76. if the pH=4.76 and the concentration of sodium acetate is 0.1M, what is the concentration of acetic acid? a)0.05...
1. The PH of Evian water is 7.4, while mountain Drew ph is 1.4. The Evian...
1. The PH of Evian water is 7.4, while mountain Drew ph is 1.4. The Evian water has; A. 0.189 times the H+ as the mountain drew B. 5.29 time lower H+ than the mountain Drew C. one million times lower H+ than the mountain drew D. 6000 times lower H+ than the mountain drew E. 6 times lower H+ than the mountain drew. 2. The PH of a solution of 0.1M Magnesium Hydroxide (milk of magnesia) can be calculated...
can you please answer 1,2, and 3 and show the steps 1. Calculate the pH of...
can you please answer 1,2, and 3 and show the steps
1. Calculate the pH of a buffer solution made by adding 20.0 mL of 0.200 M acetic acid solution with 10.0 mL of a 0.200 solution of sodium acetate. K, for acetic acid is 1.8 x 109. Assume the total volume is 30.0 mL. 2. Calculate the pH of a buffer solution made by mixing 10.0 mL of 0.20 M ammonia with 15.0 mL of 0,15 M ammonium chloride...
41.645 -113,30 Calculate the pH of a solution of 0.1M pyridine solution (CHN) with a k)...
41.645 -113,30 Calculate the pH of a solution of 0.1M pyridine solution (CHN) with a k) = 1.7 x 10-9 W Colts N 1₂O ² ColH₂NH TOH eek Lase I o.l k, CH, NAD LOH-] [Estoni C -x E .1-x x =LOH 1.7.10-9 = 0.10-0 If the base H, NON has a ky 4.4 X 10", what is the pH of a 0.05M solution of H, NOH? It is known that the K, for ammonia is 1.8 x 10-5 and...
1. Calculation: Using the Henderson-Hasselbalch equation, explain mathematically why a solution is at a pH below...
1. Calculation: Using the Henderson-Hasselbalch equation, explain mathematically why a solution is at a pH below the pKa for an acid that more than 50% of the molecules have the proton on (not off). 2. Calculation: If you have a pH of 5.5 for a weak acid with a pKa of 4.76, then is there more A- or more HA in the solution? Explain why in words using your knowledge of positive or negative log numbers.
Complete the table for an aqueous solution @ 25°C each row represents one solution Грн POH...
Complete the table for an aqueous solution @ 25°C each row represents one solution Грн POH 3.25 0.25 (H) (OH) Acidic or basic 6.14x10 12.25 1.77 9.83x102 A 0.185M solution of weak acid has a pH of 2.95. Calculate the lonization constant (K) for the acid. For this you will need to determine the relationship between the [HA], and the [H01. You're given [HA] and you'll need to find [H,0+- you can get this from pH. Just as we have...
pH of 9.2 using ammonium nitrate: pKa= 9.24 2 Introduiction The Henderson-Hasselbalch equation, or A-1 HAl relates the pH of a buffer with the pKo of the acid and the concentration of the conju...
pH
of 9.2
using ammonium nitrate: pKa= 9.24
2 Introduiction The Henderson-Hasselbalch equation, or A-1 HAl relates the pH of a buffer with the pKo of the acid and the concentration of the conjugate base A- and the monoprotic acid HA. In cq. (1), pH-_ log[H+], pK, =-log Ka, and [J]i and [JIe are the initial and equilibrium molar concentration of the Jth species, respectively. The buffering capacity of the buffer is given by [1] Ka H+ where K,e-1.0 ×...
Name Quiz Nov 14 Show all your work 1) The venom of bring ants contains formic...
Name Quiz Nov 14 Show all your work 1) The venom of bring ants contains formic acid, HCOOH (pKa 3.74 at 25C). Determine the concentration of all species present at equilibrium, the pH, and the percent dissociation of a 0.026 M solution. (Kw 1x10-1) [НСООН] [НCОО"] [H+= % dissociation pH =L_HO)
A student must make a buffer solution with a pH of 2.00. Determine which weak acid...
A student must make a buffer solution with a pH of 2.00. Determine which weak acid is the best option to make a buffer at the specified pH. O propionic acid, K = 1.34 x 10-6, 3.00 M O sodium bisulfate monohydrate, K = 1.20 x 10,3.00 M acetic acid, K, = 1.75 x 10-6, 5.00 M formic acid, K, = 1.77 x 10 , 2.00 M Determine which conjugate base is the best option to make a buffer at...
A buffer solution is able to maintain a constant pH when small amounts of acid or...
A buffer solution is able to maintain a constant pH when small amounts of acid or base are added to the buffer. Consider what happens when 1 mL of a 5 M solution is added or 0.005 mol of HCl are added to a 100.0 mL solution acetic acid buffer that contains 0.0100 mol of Acetic acid, HC,H,O,, and 0.0100 mol of sodium acetate, NaC,H,O,. The initial concentration of both the acid and the base are 0.0100 mol/ 0.1000 L...
can you please answer 1,2, and 3 and show the steps
1. Calculate the pH of a buffer solution made by adding 20.0 mL of 0.200 M acetic acid solution with 10.0 mL of a 0.200 solution of sodium acetate. K, for acetic acid is 1.8 x 109. Assume the total volume is 30.0 mL. 2. Calculate the pH of a buffer solution made by mixing 10.0 mL of 0.20 M ammonia with 15.0 mL of 0,15 M ammonium chloride...
41.645 -113,30 Calculate the pH of a solution of 0.1M pyridine solution (CHN) with a k) = 1.7 x 10-9 W Colts N 1₂O ² ColH₂NH TOH eek Lase I o.l k, CH, NAD LOH-] [Estoni C -x E .1-x x =LOH 1.7.10-9 = 0.10-0 If the base H, NON has a ky 4.4 X 10", what is the pH of a 0.05M solution of H, NOH? It is known that the K, for ammonia is 1.8 x 10-5 and...
Complete the table for an aqueous solution @ 25°C each row represents one solution Грн POH 3.25 0.25 (H) (OH) Acidic or basic 6.14x10 12.25 1.77 9.83x102 A 0.185M solution of weak acid has a pH of 2.95. Calculate the lonization constant (K) for the acid. For this you will need to determine the relationship between the [HA], and the [H01. You're given [HA] and you'll need to find [H,0+- you can get this from pH. Just as we have...
pH
of 9.2
using ammonium nitrate: pKa= 9.24
2 Introduiction The Henderson-Hasselbalch equation, or A-1 HAl relates the pH of a buffer with the pKo of the acid and the concentration of the conjugate base A- and the monoprotic acid HA. In cq. (1), pH-_ log[H+], pK, =-log Ka, and [J]i and [JIe are the initial and equilibrium molar concentration of the Jth species, respectively. The buffering capacity of the buffer is given by [1] Ka H+ where K,e-1.0 ×...
Name Quiz Nov 14 Show all your work 1) The venom of bring ants contains formic acid, HCOOH (pKa 3.74 at 25C). Determine the concentration of all species present at equilibrium, the pH, and the percent dissociation of a 0.026 M solution. (Kw 1x10-1) [НСООН] [НCОО"] [H+= % dissociation pH =L_HO)
A student must make a buffer solution with a pH of 2.00. Determine which weak acid is the best option to make a buffer at the specified pH. O propionic acid, K = 1.34 x 10-6, 3.00 M O sodium bisulfate monohydrate, K = 1.20 x 10,3.00 M acetic acid, K, = 1.75 x 10-6, 5.00 M formic acid, K, = 1.77 x 10 , 2.00 M Determine which conjugate base is the best option to make a buffer at...
A buffer solution is able to maintain a constant pH when small amounts of acid or base are added to the buffer. Consider what happens when 1 mL of a 5 M solution is added or 0.005 mol of HCl are added to a 100.0 mL solution acetic acid buffer that contains 0.0100 mol of Acetic acid, HC,H,O,, and 0.0100 mol of sodium acetate, NaC,H,O,. The initial concentration of both the acid and the base are 0.0100 mol/ 0.1000 L...
Most questions answered within 3 hours.
-
2. Use the following information in the table to answer the
following questions. (Numbers are in...
asked 2 minutes from now -
The rate constant of a first-order reaction is 2.95 × 10−4 s−1
at 350.° C. If...
asked 35 seconds ago -
The fuel economy of a 2011 Lexus RX 350 2wd 6 cylinder 3.5 L
automatic 5...
asked 5 minutes ago -
i.
the synthesized compund 2-bromo-butanal i have a IR peak at about
3200 and one at...
asked 5 minutes ago -
A
752 mL sample of water was placed in a 1000 gram pan of aluminum.
The...
asked 17 minutes ago -
1.In the context of chelation, what does binding strength mean?
What happens at the molecular level...
asked 9 minutes ago -
Describe two obstacles that makes fixing atmospheric nitrogen
difficult.
asked 29 minutes ago -
Evelyn incorporates her sole proprietorship, transferring it to
newly formed Papaya Corporation. The assets transferred have...
asked 15 minutes ago -
Assume that in a hydrogen atom, the electron circles the nucleus
in a circle of radius...
asked 24 minutes ago -
1 point) Given the significance level α=0.01 find the following:
(a) left-tailed z value z= (b)...
asked 18 minutes ago -
Calculate the expected value, the variance, and the standard
deviation of the given random variable X....
asked 20 minutes ago -
T
F 53) Most differences
between human groups are the result of biology rather than
culture....
asked 33 minutes ago