TITLE DATE C. Will WHy HS be acidic or basic in H₂O? kb of NH3 7 1.76 x 10-5 2 Kai H S = 9 × 10-8 Jad greatest vale is 1.76 × 105 Solution IS basic 2. C₁₂ H18 ONY scle Ka = 3.37 2107 ① Find pH = 3,50 PH = 10-3.5 46= kb= 1,0×10 3.37x107 -14 *- 3.0 x10 + H₂O C→ C₁₂ H₁, UNY SCI₂ -log [H3O+] 3.50 = -log C H₂01 H30 = CH2O = 3,220 Xô Galaxy S21 Ultra 5G SQUARE = i 939 out tion 900 Shoutd 7. Thiamine hydrochloride (C12H18ON4SCI2) is a water soluble form of thiamine (vitamin B1; Ka = 3.37 x 107). How many grams of the hydrochloride must be dissolved in 10.00 mL of water to give a pH of 3.50? C12H18ON4SCl2 + H2O C12H17ON4SCl2 + H3O+ 8. What is the pH of a solution containing 33 g of Na3PO4 per liter? What is the [OH-] of this solution? See necessary Ka values above in problem 1. POU 3- + 7 Н2О = 4ром 2- Kb = kw +04 Ka Und NPO 33 Na Poy 163.74 mil Naz pou IL S -20129 M PO³- Ice The 1.0×10-14 4.2 x10-13 =2.4×10-2 48 | Page V= 10.00μL

TITLE DATE C. Will WHy HS be acidic or basic in H₂O? kb of NH3 7 1.76 x 10-5 2 Kai H S = 9 × 10-8 Jad greatest vale is 1.76 × 105 Solution IS basic 2. C₁₂ H18 ONY scle Ka = 3.37 2107 ① Find pH = 3,50 PH = 10-3.5 46= kb= 1,0×10 3.37x107 -14 *- 3.0 x10 + H₂O C→ C₁₂ H₁, UNY SCI₂ -log [H3O+] 3.50 = -log C H₂01 H30 = CH2O = 3,220 Xô Galaxy S21 Ultra 5G SQUARE = i 939 out tion 900 Shoutd 7. Thiamine hydrochloride (C12H18ON4SCI2) is a water soluble form of thiamine (vitamin B1; Ka = 3.37 x 107). How many grams of the hydrochloride must be dissolved in 10.00 mL of water to give a pH of 3.50? C12H18ON4SCl2 + H2O C12H17ON4SCl2 + H3O+ 8. What is the pH of a solution containing 33 g of Na3PO4 per liter? What is the [OH-] of this solution? See necessary Ka values above in problem 1. POU 3- + 7 Н2О = 4ром 2- Kb = kw +04 Ka Und NPO 33 Na Poy 163.74 mil Naz pou IL S -20129 M PO³- Ice The 1.0×10-14 4.2 x10-13 =2.4×10-2 48 | Page V= 10.00μL

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 107E: A typical vitamin C tablet (containing pure ascorbic acid, H2C6H6O6) weighs 500. mg. One vitamin C...

See similar textbooks

Question

100%

I am not sure how to get kb and I want to see if I am on the right track for this equation ... Number 8

TITLE
DATE
C. Will
WHy HS
be acidic
or basic in H₂O?
kb
of NH3
7 1.76 x 10-5
2
Kai H
S
= 9 × 10-8
Jad
greatest vale
is 1.76 × 105
Solution
IS
basic
2.
C₁₂ H18 ONY scle
Ka = 3.37 2107
①
Find
pH = 3,50
PH
=
10-3.5
46=
kb=
1,0×10
3.37x107
-14
*-
3.0 x10
+ H₂O C→ C₁₂ H₁, UNY SCI₂
-log [H3O+]
3.50
= -log C H₂01
H30
= CH2O = 3,220 Xô
Galaxy S21 Ultra 5G
SQUARE =
i
939

out
tion
900
Shoutd
7. Thiamine hydrochloride (C12H18ON4SCI2) is a water soluble form of thiamine (vitamin B1; Ka =
3.37 x 107). How many grams of the hydrochloride must be dissolved in 10.00 mL of water to
give a pH of 3.50?
C12H18ON4SCl2 + H2O C12H17ON4SCl2 + H3O+
8. What is the pH of a solution containing 33 g of Na3PO4 per liter? What is the [OH-] of this
solution? See necessary Ka values above in problem 1.
POU
3-
+
7
Н2О = 4ром 2-
Kb = kw
+04
Ka
Und NPO
33 Na Poy 163.74 mil Naz pou
IL
S
-20129 M PO³-
Ice The
1.0×10-14
4.2 x10-13
=2.4×10-2
48 | Page
V= 10.00μL

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step by step

Solved in 2 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Similar questions

Acrylic acid (CH29CHCO2H) is a precursor for many important plastics. Ka for acrylic acid is 5.6 105. a. Calculate the pH of a 0.10-M solution of acrylic acid. b. Calculate the percent dissociation of a 0.10-M solution of acrylic acid. c. Calculate the pH of a 0.050-M solution of sodium acrylate (NaC3H3O2).
Find [OH+], [OH-] and the pH of the following solutions. (a) 30.0 mL of a 0.216 M solution of HCI diluted with enough water to make 125 mL of solution. (b) A solution made by dissolving 275 mL of HBr gas at 25C and 1.00 atm in enough water to make 475 mL of solution. Assume that all the HBr dissolves in water.
Consider a 0.67-M solution of C2H5NH2 (Kb = 5.6 104). a. Which of the following are major species in the solution? i. C2H5NH2 ii. H+ iii. OH iv. H2O v. C2H5NH3+ b. Calculate the pH of this solution.
A typical vitamin C tablet (containing pure ascorbic acid, H2C6H6O6) weighs 500. mg. One vitamin C tablet is dissolved in enough water to make 200.0 mL of solution. Calculate the pH of this solution. Ascorbic acid is a diprotic acid.
Amantadine, C10H15NH2, is a weak base used in the treatment of Parkinsons disease. Its conjugate acid has Ka = 7.9 1011. Calculate the pH of a 0.0010-M aqueous solution of amantadine at 25 C.
Consider 50.0 mL of a solution of weak acid HA (Ka = 1.00 106), which has a pH of 4.000. What volume of water must be added to make the pH = 5.000?
Consider two weak acids, HA (MM=138g/mol)and HB (MM=72.0g/mol). A solution consisting of 11.0 g of HA in 745 mL has the same pH as a solution made up of 5.00 g of HB in 525 mL. Which of the two acids is stronger? Justify your answer by an appropriate calculation.
Sketch two graphs: (a) percent dissociation for weak acid HA versus the initial concentration of HA ([HA]0) and(b) H+ concentration versus [HA]0. Explain both.
For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen atom? b. the electronegativity of the element bonded to the oxygen atom that bears the acidic hydrogen? c. the number of oxygen atoms? How does the strength of a conjugate base depend on these factors? What type of solution forms when a nonmetal oxide dissolves in water? Give an example of such an oxide. What type of solution forms when a metal oxide dissolves in water? Give an example of such an oxide.
Calculate the pH of a 0.12 M aqueous solution of the base aniline, C6H5NH2(Kb=4.01010). C6H5NH2(aq)+H2O(l)C6H5NH3+(aq)+OH(aq)
The following illustration displays the relative number of species when an acid, HA, is added to water. a. Is HA a weak or strong acid? How can you tell? b. Using the relative numbers given in the illustration, determine the value for Ka and the percent dissociation of the acid. Assume the initial acid concentration is 0.20 M.
You are asked to calculate the H+ concentration in a solution of NaOH(aq). Because sodium hydroxide is a base, can we say there is no H+. since having H+ would imply that the solution is acidic?