* Asiacell li.uo 9:53A docs.google.com40%מ>3.2 ml2.8 mlThe PH of 0.0296M HA ( Ka 8.4 *10-9) plus0.1026 M NaA is4.3 O28.67.5 Oml of 0.1M of weak acid (Ka =1.7 * 10-5) 50was titrated with 0.1M NaOH the pH afteraddition of 50ml NaOH is10.3 O7 O8.5.2

The question is based on the concept of PH calculations. we have been given a weak acid and its…

Science

Chemistry

The PH of 0.0296M HA ( Ka 8.4 *10-9) plus * . . 0.1026 M NaA is 4.3 2 O 8.6 7.5 O

The PH of 0.0296M HA ( Ka 8.4 10-9) plus . . 0.1026 M NaA is 4.3 2 O 8.6 7.5 O

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: Ascorbic acid (HC6H706) is a weak monoprotic acid (HA); A) Calculate the pH of a solution produced…

A: The above question is from titration of weak acid with a strong base.

Q: You have an aliquot of 10 mL of 0.1097 mol/L phosphoric acid. The ka values for phosphoric acid are…

A: Volume of phosphoric acid = 10 mLMolarity of phosphoric acid sample = 0.1097 mol/LVolume of NaOH…

Q: Determine the pH at the point in the titrátion of 40.0 mL of 0.200 M HC4H,O2 with 0.100 M Sr(OH)2…

A: Base dissociation constant , Kb represents basicity in a solution. For a dissociation of base (B) in…

Q: 10) You make a solution that has a final concentration of 0.400 M acetic acid and 0.350 M sodium…

Q: 2. Calculate the pH at 25 °C of a solution that is 0.3 M in NaH2AsO4 at 25 °C (Kal =5.8 x 10, Ka2 =…

Q: 7. Calculate the pH value when 10.0mL of 1.0M HCI is added to the solution in question 5. (pH…

A: Answer-6Buffer solution is a type of solution that resists the change in its pH on adding small…

Q: Calculate the pH of a solution prepared by adding 30.0 mLs of 0.20 M HCl to 50.0 mLs of 0.10 M…

A: Given: Concentration of HCl = 0.20 M Volume of HCl solution = 30.0 mL = 0.030 L…

Q: 1. a. What is the pH of a solution prepared by adding 25.0 mL of 0.10 M acetic acid (Ka = 1.8 x…

Q: 23). A solution with a pOH of 4.3 has a [H] of a). 6.8 x 10 M. c) 4.8 x 10* M. b). 3.2 х 10+ м. d)…

A: Given data: The pOH value = 4.3. To find: [H+]

Q: What is the pH of a 1.75 M solution of KX (Kb of X is 1.22 x 10°) (Please show the final result with…

A: Answer: 9.66 Weak base can't dissociate completely, it's pOH = 1/2 (PKb - logC)

Q: You have an aliquot of 12 mL of 0.1024 mol/L phosphoric acid. The ka values for phosphoric acid are…

A: The objective of the question is to calculate the resultant pH when 12 mL of 0.1024 mol/L phosphoric…

Q: Calculate the volume, in milliliters, of 0.170 M NaOH that must be added to 403 mL 0.0479 M…

A: Using Henderson hasselbalch equation we can figure out the volume of NaOH solution required.

Q: Calculate the pH of the follo 0.39 M NH4CI (рКp fo O a. 2.57 O b.4.83 с. 9.67 O d.4.33 O e. none of…

A: Given, pKb = 4.74 Concentration of Salt(C)= 0.39 M It is salt of weak base -strong acid type salt .…

Q: 12. Sodium Azide (NaN3) is sometimes added to water to kill bacteria. Calculate the pH of a 0.010…

A: Step 1: The chemical equation for the ionization of the azide ion in water isBased on the given…

Q: 6. Calculate the hydroxide ion concentration [OH] in an aqueous solution that contains [H*] = 2.5 x…

Q: Calculate the pH, [H2L*], [HL], [L] for each solution of the amino acid proline (Kal = 1.12 x 102…

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: How many grams of BHCl (acidic salt, 65.47 g/mol) would need to be added to 435 mL of 1.79 M B (a…

A: The question is based on the concept of buffer solution. A buffer is a solution which resist any…

Q: You have an aliquot of 10 mL of 0.1094 mol/L phosphoric acid. The ka values for phosphoric acid are…

A: The objective of this question is to calculate the resultant pH of a solution after mixing…

Q: Calculate the pH for each of the cases in the titration of 25.0 mL of 0.170 M pyridine, C, H, N(aq)…

A: we need to calculate the pH of the given solutions

Q: How many grams of BHCl (acidic salt, 69.83 g/mol) would need to be added to 490 mL of 1.5 M B (a…

A: The pH of the solution is the power of protons in the solution. While pOH is related to the basicity…

Q: What is the pH of a 0.375 L solution made with and 25.00 mL of 5.50 M HBRO (K, = 2.3 x 10 ) 2.775 g…

Q: 3. What is the pH of a 1.15 M solution of methanoic acid? K = 1.8 x 104

Q: What is the pH of a solution containing 0.1279 M HOCN and 0.1517 M KOCN? Ka = 3.50e-4. 10.544…

A: Acid, [HOCN] = 0.1279 M Salt, [KOCN] = 0.1517 M Ka = 3.50 × 10-4

Q: A 5.50 g sample of a weak acid with K₁ = 1.3 x 10-4 was combined with 5.20 mL of 6.00 M NaOH and the…

Q: What is the pH of a soln which is 0.5 M NH3 and 0.075M NH4Cl? (kb=1.8x10-5)

A: The solution of NH3 and NH4Cl will form a buffer solution and the pH of a buffer solution is…

Q: Calculate the pH of a solution which contains 0.814 moles of CH3NH2 and 0.788 moles of CH3NH3CI. Kb…

Q: pH = 3.4 What are the equilibrium concentrations of H₂A and A²- in this soluti [H₂A] = [A²-] =…

Q: f the K, of a monoprotic weak acid is 2.7 x 10-6, what is the pH of a 0.48 M solution of this acid?…

Q: A drinking water source is found to be excessively "hard" with high levels of calcium and magnesium…

A: Given : water source is found to be excessively "hard" with high levels of calcium and magnesium…

Q: Complete the balanced neutralization equation for the reaction below: H2SO:(aq) + Mg(OH):(aq) –

A: To complete the balanced neutralization reaction H2SO4 (aq) + Mg (OH)2 (aq) ----------->

Q: //app.101edu.co Question 5 of 7 Calculate the pH when 61.0 mL of 0.150 M KOH is mixed with 20.0 mL…

Q: What is the pH of 100.0 mL of 0.10 M HNO;? nooulos M 005.0s ai nois 01 x 02.1 g CH'COOH What is the…

A: pH = -log [H+]

Q: A.) Calculate the pH of a 0.359 M aqueous solution of hydrofluoric acid (HF, Ka = 7.2×10-4) and the…

Q: 3. Calculate the pH of a 0.400 M KC2H3O2 (Ka for HC2H3O2 is 1.8 x 10-5)

A: In this question we have to tell the PH of the solution.

Q: Calculate the pH of a solution that is 0.0890 M in a. NaH₂PO4 (Kal = 7.11 x 10³, K-6.32 × 108). pH-…

A: The objective of the question is to calculate the .

Q: A buffer solution is 0.361 M in KH2PO4 and 0.223 M in K2HPO4. If Ka for H2PO4 is 6.2 x 10-8, what is…

A: Henderson - Hasslebalch equation is given below pH = pKa + log[conjugate base][acid] And Ka = acid…

Q: What

A: Buffer is the solution of mixture of weak acid/weak base with its salt of strong base/strong acid

Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

* Asiacell li.
uo 9:53
A docs.google.com
40%מ>
3.2 ml
2.8 ml
The PH of 0.0296M HA ( Ka 8.4 *10-9) plus
0.1026 M NaA is
4.3 O
2
8.6
7.5 O
ml of 0.1M of weak acid (Ka =1.7 * 10-5) 50
was titrated with 0.1M NaOH the pH after
addition of 50ml NaOH is
10.3 O
7 O
8.
5.2

Expert Solution

This question has been solved!

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

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 1 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

5. A buffer solution contains 10.0 mmol of formic acid (HCOOH) and 15.0 mmol of formate (HCO0). If the solution pH is 3.95, then what is the Ka of formic acid? (а) 7.5 х 10-5 (b) 1.1 х 104 (c) 4.1 x 102 (d) 1.7 x 10-4
None
Calculate the pH of the solution formed when 0.00 mL of 0.0440 M NaOH is added to 48.20 mL of 0.0440 M weak acid (Ka = 2.90e-05). 2.47e+00 5.07e+00 The answer is not shown. 4.59e-01 2.95e+00
What is the pH of a 0.600 M solution of HSo, (Ka = 6.6 × 10°)? (Please show your answers with 3 sig figs.) | M 1 3 4 6. C 7 8 9 +/- x 100
Molecule A C1819 NOS pKa = 9.3 Which of these pairs of species is more abundant in a solution of molecule C with a pH = 8 ? C18H19NOS, OH C18H20NOS+, OH- C18H19NOS, H3O+ X C18H20NOS+, H3O+
If a 0.552M HCl caq) solution is used by a scientist to titrate 10.00mL of a weak base, based curve (shown below), what base? write your the titration the concentration of the auswer with 4 decitual places. pH Curve OM is 12 10 8 6 4 2 0 5:0 2 1.5 n 3 3.5 A Volume of Titrant / mL 7.5 8 8.5
Macmillan Leashilg ao At 25 °C, how many dissociated OH ions are there in 1293 mL of an aqueous solution whose pH is 1.81? 7 101 number of OH ions: R L A: 0 15 % 5 T a f6 6 30 17 & Y ] 7 18 D ➡+ 8 19 即可 9 K fio ▶II O O L fn ►►I 62°F ») 112 + P [ 7 insert ← ions 3:33 PM 10/5/2022 prt sc backspac 1 1
The pK, of a particular weak acid is 5.17. What is the pH of the weak acid solution when exactly half of the acid is neutralized? pH = Prev 2 of 5 Next >
A solution contains 0.177 M potassium hypochlorite and 0.337 M hypochlorous acid ( Ka 3.5 × 10-³). The pH of this solution is = Submit Answer Retry Entire Group 2 more group attempts remaining
Calculate the pH of a solution that is 0.66 M HF and 1.00 M KF. к, 3 7.2 х 10-4 pH =
Calculate the pH of a solution that is 0.70 M in HF ( Ka= 7.2 × 104) and 0.66 M in NaF. а. 3.40 O b.0.12 О с. 3.26 O d. 10.74 О е. 3.12