### Lab Report #6-2-4: ### 0.1 M Na₃PO₄ Solution, Using the Given pH Data, Calculate the Value of (Ka or Kb)**Multiple Choice Options:**1. 1.0 x 10⁻⁴2. 6.2 x 10⁻⁵3. 6.2 x 10⁻⁴4. 1.0 x 10⁻⁵---#### Explanation:The goal of this lab report is to determine the value of the acid dissociation constant (Ka) or the base dissociation constant (Kb) for a 0.1 M solution of sodium phosphate (Na₃PO₄) using the provided pH data. The result should be one of the given multiple-choice options.1. **1.0 x 10⁻⁴**2. **6.2 x 10⁻⁵**3. **6.2 x 10⁻⁴**4. **1.0 x 10⁻⁵**> To solve this, use the pH data and the formula for calculating Ka or Kb. Apply the concentrations and related equations according to the provided conditions. The correct answer will be among the options listed.This multiple-choice question is a part of a series of exercises meant to facilitate the understanding of chemical equilibria in solutions, specifically focusing on weak acids and bases and their dissociation constants. ### pH Values of Various SolutionsThe following table displays the pH values of different solutions, both common and chemical, and provides insight into their acidic or basic nature. | **Solutions** | **pH values** ||---------------------|---------------|| H₂O (unboiled) | 3.5 || H₂O (boiled) | 7.0 || NaCl | 7.0 || NaC₂H₃O₂ | 9.1 || NH₄Cl | 4.5 || NaHCO₃ | 9.5 || Na₃PO₄ | 11.9 || Na₂CO₃ | 11.0 |#### Explanation:- **H₂O (unboiled)**: pH of 3.5, indicating it is slightly acidic.- **H₂O (boiled)**: pH of 7.0, indicating neutrality.- **NaCl (Sodium Chloride)**: pH of 7.0, also neutral.- **NaC₂H₃O₂ (Sodium Acetate)**: pH of 9.1, indicating it is basic.- **NH₄Cl (Ammonium Chloride)**: pH of 4.5, indicating it is acidic.- **NaHCO₃ (Sodium Bicarbonate)**: pH of 9.5, indicating it is basic.- **Na₃PO₄ (Sodium Phosphate)**: pH of 11.9, showing it is strongly basic.- **Na₂CO₃ (Sodium Carbonate)**: pH of 11.0, indicating it is strongly basic.This table serves as an educational resource to better understand the pH scale and the nature of various common substances.

The question is based on the concept of salt hydrolysis . we have to calculate the dissociation…

Answered: Lab Report #6-2-4: 0.1 M NagPO4…

Lab Report #6-2-4: 0.1 M NagPO4 solution, using the given pH data, calculate value of (Ka or Kb) O 1.0 x 10-4 O 6.2 x 10-5 O 6.2 x 10-4 1.0 x 10-5

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: Q1//A solution of o.1 M of BX salt with pH=9.5, the HX is weak acid and BOH a strong base. Calculate…

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

Q: Q-4- Explain in detail Two of the following. 1- Calculate the pH of 0.1 M ammonium chloride. pkb…

A: The question is based on the concept of chemical equilibrium and solutions. we have to calculate pH…

Q: You plan to make a buffer solution with sulfurous acid (H₂SO3) and it undergoes dissociation…

A: To make a buffer solution at pH 7.040, we can use the Henderson-Hasselbalch equation: pH = pKa +…

Q: Calculate the pH when 20.0 mL of 0.150 M KOH is mixed with 27.0 mL of 0.300 M HBrO (Ka = 2.5 x 10-⁹)

A: Data

Q: O3// Calculate the sodium acetate concentration that used in preparing a buffer solution with…

Q: Ka for hypochlorous acid HCIO is 3.0 x 10-8. Calculate the pH after the addition of 15.0o mL of…

A: Initial moles of HClO = Molarity ×Volume = 0.100 M × 40.0 mL = 4mmoles Initial moles of NaOH =…

Q: What is the equilibrium concentration of H2C2O4 in a .542 M oxalic acid H2C2O4 solution? For oxylic…

Q: Q-4- Explain in detail Two of the following. 1- Calculate the pH of 0.1 M ammonium chloride. pkb…

A: The question is based on the concept of pH of the solution. it is defined as a negative logarithm…

Q: 0.1 M NH4CI solution, using the given pH data, write net-ionic equation for hydrolysis: NH4* + H20 +…

A: Salt hydrolysis :- The interaction of cation or anion or both of a salt to form an acidic or basic…

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: 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: Which of the following solutions would be expected to have a pH of 7.00?

Q: What is the pH of a solution that is 0.048 M in HA and also 0.0042 M in NaA? (Ka = 4.1 %3D x 10-6)

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: The hydroxide ion concentration in a solution of NaOH is 7.6 x 10-¹ M at 25 °C. What is the pH of…

Q: You have an aliquot of 10 mL of 0.1022 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 concentrations of ALL the ions present in a 0.0300M solution of carbonic acid (H2CO3…

A: H2CO3 is a weak acid. It is form from the reaction of CO2 with water. Given data: Ka1 = 4.2×10-7…

Q: Consider 0.2 M H2A (Given Ka1= 1x10^-5, Ka2=1x10^-9). Calculate the Concentration of HA^- at pH =5…

A: We know strong acid are those acid which dissociate 100% while weak acid are those which does not…

Q: Calculate the pH of a 0.018M H2SO4 solution that has a Ka1=strong and Ka2=1.2•10-2

Q: What mass of NaA (MW=100 g/mole) must be added to a 100.0 ml of a 0.1 M solution of HA (Ka=1x10-5)…

Q: Phosphoric acid is a triprotic acid with the Ka values of 7.25 10-3, 6.31 10-8 and 3.98 10-13…

A: Millimoles of H3PO4 taken =Molar concentration of acid×Volume of acid=0.1000 M×25 mL=2.5 mmol

Q: Calculate the ratio of CH3CO0' to CH3COOH required to buffer a solution with a pH of 4.00. Use Ka…

A: Acetic acid (CH3COOH) is weak acid which dissociates partially in water.…

Q: 7-)

Q: For HF, Ka = 7.2 x 10-4. For a 0.15 M solution of NaF, Find pH and pOH

A: The Bronsted-Lowry acid-base theory was purposed by Bronsted and Lowery is called Bronsted-Lowry…

Q: Question 20 Calculate the pH of a buffered aqueous solution consisting of 0.07 M Li₂HPO4 and 0.085 M…

A: Li2HPO4 = 0.07 M Li2PO4 = 0.085 M Ka = 4.84 x 10 —13

Q: Calcula HNO2 ( A typic (acetyls Ka = 3. %3D 300ML the per

A: Concept pH of the solution can be calculated as: pH= - log [H+]

Q: Determine the Ka value [H +]eq Solution 1 3.98 X 10-3 M Solution 2 6.03 X 10-4 M Solution 3…

A: Hello. Since your question has multiple sub-parts, we will solve the first three sub-parts for you.…

Q: Calculate the expected pH of a buffer prepared by dissolving 1.3 mols of acetic acid and 0.4 mols of…

A: Given buffer solution pH calculated by using formula.

Q: Select any systems that could be used to buffer a solution at a pH of 6. Mark all appropriate…

Q: 3, Calculate the pH of a solution prepared by mixing 150.0 mL of 0.200 M hydrobromic acid and 150.00…

A: (3)

Q: Consider the titration of 40.0 mL of 0.18 M H3A (Kal = 1.9 × 10-4, Ka₂ = 1.2 × 10-8, Kaz KOH. a.…

A: A 40.0 mL of 0.18 M weak triprotic acid H3A is titrated with 0.18 M KOH. The acid the dissociation…

Q: 9. Calculate the pH of a 0.20 M solution of iodic acid (HIO3 and K₂ = 0.17). [78] 10. Calculate the…

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

Q: how many liters of 0.54 monoprotic acid should be added to 685000 L of water with ph 7 to reach ph…

A: Given the desired pH of the acid solution with water = 5.2 Frist we have to find the [H+(aq)] from…

Q: What is the percent ionization of acetic acid (CH3COOH) in a solution that contains 0.10 M acetic…

A: Ionic solids are metal salts. They formed when metals form an ionic bond with non-metals. Ionic…

Q: Calculate the pH of a solution prepared by dissolving 3.90 g of sodium acetate (NAC2H3 of solution.…

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

Q: Q1//A solution of 0.1 M of BX salt with pH=9.5, the HX is weak acid and BOH a strong base. Calculate…

Q: alculate the pH in a solution which is made when 23.0 mL of 0.12 M NH3 (Kb = 1.8 x 10-5) is added to…

Q: Calculate the pH of Ka for HCHO₂ is 1.8 × 10 a 0.10 M Na CHO₂ solution. -4

Q: Consider the titration of a 29.0 mL sample of 0.170 mol L-1 CH₂COOH (K=1.3 x 10-5) with 0.120 mol…

A: Since you have posted a question with multiple sub-parts, we will provide the solution only to the…

Q: Determine the Ka value [H +]eq Solution 5 4.68 X 10-10 M Directions Take a 30.0 mL sample…

A: The concentration of hydroxyl ion is calculated as follows:

Q: Calculate the pH of a solution containing 0.20 M HC2H302 and 0.25 M NaC2H3O2. The Ka for HC2H3O2 is…

A: pKa = -log Ka = - log (1.8×10-5) = 4.74

Question

### Lab Report #6-2-4:
### 0.1 M Na₃PO₄ Solution, Using the Given pH Data, Calculate the Value of (Ka or Kb)

**Multiple Choice Options:**

1. 1.0 x 10⁻⁴
2. 6.2 x 10⁻⁵
3. 6.2 x 10⁻⁴
4. 1.0 x 10⁻⁵

---

#### Explanation:
The goal of this lab report is to determine the value of the acid dissociation constant (Ka) or the base dissociation constant (Kb) for a 0.1 M solution of sodium phosphate (Na₃PO₄) using the provided pH data. The result should be one of the given multiple-choice options.

1. **1.0 x 10⁻⁴**
2. **6.2 x 10⁻⁵**
3. **6.2 x 10⁻⁴**
4. **1.0 x 10⁻⁵**

> To solve this, use the pH data and the formula for calculating Ka or Kb. Apply the concentrations and related equations according to the provided conditions. The correct answer will be among the options listed.

This multiple-choice question is a part of a series of exercises meant to facilitate the understanding of chemical equilibria in solutions, specifically focusing on weak acids and bases and their dissociation constants.

### pH Values of Various Solutions

The following table displays the pH values of different solutions, both common and chemical, and provides insight into their acidic or basic nature.

| **Solutions** | **pH values** |
|---------------------|---------------|
| H₂O (unboiled) | 3.5 |
| H₂O (boiled) | 7.0 |
| NaCl | 7.0 |
| NaC₂H₃O₂ | 9.1 |
| NH₄Cl | 4.5 |
| NaHCO₃ | 9.5 |
| Na₃PO₄ | 11.9 |
| Na₂CO₃ | 11.0 |

#### Explanation:
- **H₂O (unboiled)**: pH of 3.5, indicating it is slightly acidic.
- **H₂O (boiled)**: pH of 7.0, indicating neutrality.
- **NaCl (Sodium Chloride)**: pH of 7.0, also neutral.
- **NaC₂H₃O₂ (Sodium Acetate)**: pH of 9.1, indicating it is basic.
- **NH₄Cl (Ammonium Chloride)**: pH of 4.5, indicating it is acidic.
- **NaHCO₃ (Sodium Bicarbonate)**: pH of 9.5, indicating it is basic.
- **Na₃PO₄ (Sodium Phosphate)**: pH of 11.9, showing it is strongly basic.
- **Na₂CO₃ (Sodium Carbonate)**: pH of 11.0, indicating it is strongly basic.

This table serves as an educational resource to better understand the pH scale and the nature of various common substances.

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 1

VIEW

Step 2

VIEW

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

Calculate the pH of an aqueous solution that is 3.24 x 10-1 M oxopropanoic acid and 0.101 M sodium oxoproanoate? [HINT: MW sodium oxopropanoate = 110.05 g/mol; Kaoxopropanoic acid = 3.30 x 10-3]
Calculate the pH of a solution that is 0.15 M H2CO3 and 0.10 M NaHCO3 (Ka = 4.3 X 10-7). 6.38 6.19 0.176 6.54 0.352
2-
You have an aliquot of 10 mL of 0.1042 mol/L phosphoric acid. The ka values for phosphoric acid are 6.9 *10-3, 6.2*10-8 and 4.8 *10-13. If you mix 26 mL of 0.1064 mol/L NaOH what is the resultant pH? Answer to two decimal places.
Calculate the following: a- A weak acid CHA) solution has a pH of 2.25. Find the acíd iconization constant, Ka 0.125 M b- Find the [OH-] and öH of a 0.127 M NH 3 olution. The Kb for NH 8 is 1.8x10-5
lues if heeded for this question. A buffer solution is 0.401 M in H½S and 0.278 M in KHS. If Ka1 for H2S is 1.0 × 10-7, what is the pH of this buffer solution? pH = Submit Answer Retry Entire Group 9 more group attempts remaining тес Not Visited 2red Зred Previous Next ent Save and Exit Cengage Learning | Cengage Technical Support MacBook Air .. R. 吕0 DII F1 F2 F3 F4 F5 F6 F7 F8 2$ & * %23
What is the equilibrium concentration of H2C2O4 in a 0.170 M oxalic acid, H2C2O4, solutio For oxalic acid, Kal = 5.6 × 10-2 and Ka2 = 5.1 × 10-5. 9.6 × 10-2 M 9.8 × 10 2 M O 1.7 x 101 M O 5.1 x 10-5 M O 7.4 x 10-2 M
4-)
What is a pH of a solution resulting from the addition of 14.78 mL of 0.1392 M NaOH to 28.99 mL of 0.1950 M HC7H5O2? Ka = 6.300e-5. 4.3971 3.9580 2.4553 9.6724
What is the pH of the solution when Yolanda has added 60.0 mL of 0.10 M LIOH to the 40.0 mL of 0.40 M HBrO? KaHA = 2.0 x 10-⁹ pH = [?] pH @ 60 mL base Enter
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