Question: Calculate dissociation per mole of NaHSO4 in water. Data Given from this Enthalpy of Neutralization for NaHSO4 experiment: Volume of NaHSO4 = 50 mL & Conc of NaHSO4 = 1.2M Volume of NaOH = 50 mL & Conc of NaOH = 1.5M Mass of combined solution = 100 g Ti of NaHSO4 = 23.4 degrees Celsius and Tf of NaHSO4 = 32 degrees Celsius Moles of NaHSO4 = 1.2M x 50.0E-3 L = 0.060 mol Enthalpy of neutralization per mole of NaHSO4 = -60 KJ/mol

Question: Calculate dissociation per mole of NaHSO4 in water. Data Given from this Enthalpy of Neutralization for NaHSO4 experiment: Volume of NaHSO4 = 50 mL & Conc of NaHSO4 = 1.2M Volume of NaOH = 50 mL & Conc of NaOH = 1.5M Mass of combined solution = 100 g Ti of NaHSO4 = 23.4 degrees Celsius and Tf of NaHSO4 = 32 degrees Celsius Moles of NaHSO4 = 1.2M x 50.0E-3 L = 0.060 mol Enthalpy of neutralization per mole of NaHSO4 = -60 KJ/mol

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: Which of these mixtures represents a shift in the forward direction? Select all apply

A: Here equilibrium established in the reaction.

Q: The titration of 25.0 mL of an unknown concentration H₂SO4 solution requires 83.6 mL of 0.12 M LIOH…

Q: REPORT SHEET Determination of the Dissociation Constant of a Weak Acid B. Standardization of Sodium…

A: The following reaction takes place. in which one mole of KHP reacts with one mole of NaOH…

Q: A 25.0 mL solution of HBr is neutralized with 18.7 mL of 0.230 M Ba(OH)2. What is the concentration…

Q: Calculate the pH of a solution that contains 0.375 M HCN and 0.400 M NaCN Data: Ka of HCN = 6.2 x…

A: Buffer solution: The solution that resists the change in pH is known as a buffer solution. The…

Q: Data Table: Room Temperature Saturated Solution (25 °C) 100 °C Saturated Solution Volume of…

A: •CONCEPT:--Here in titration we add "HCl" in solution of Calcium hydroxide to find out its…

Q: 2. Oxalic acid (a diprotic acid HOOCCOOH; pKal 1.25 and pKa2 = 4.28 at 25°C) is added to pure water…

A: The objective of the question is to determine the final pH of a solution of oxalic acid in water and…

Q: Please correct answer and don't use hand rating

A: Given: Acid (strong): HNO3 Acid volume, Vacid = 80.0 mLMolarity of acid, Macid = 0.770 M Base…

Q: 2. 15.0 mL HNO3 was titrated to equivalence with 60.0 mL of 0.020 NAOH, What is the concentration of…

A: Given : Volume of HNO3 = 15.0 mL Molarity of NaOH = 0.020 M Volume of NaOH = 60.0 mL To…

Q: Full Screen Accessibility While titrating 50.0 mL of a 0.582 M solution of HCI with a solution…

A: Acid-base titration: Titration is a method to determine the concentration of unknown acid by using…

Q: pH =-log[H,O'] 14 pH+ pOH QUESTION 7 What is the molar solubility of YF3 in water? Kep =8.62x1021…

A: I will give Solution for first Question ( Question 7 ) in details. In this question, you will…

Q: For a water sample with a bicarbonate ion concentration of 50 mg/L and a CO2 content of 30 mg/L: a)…

Q: A 100 mL water sample requires 7 ml of 0.1N HCI to titrate to the phenolphthalein endpoint (pH 8.3)…

A: Solution- Alkalinity of CaCO3

Q: 100.0 mL sample of natural water was titrated with NaOH. The titration required 10.25 mL of 0.1075 M…

Q: QUESTION 16 What is the pH of a 0.20 M solution of the weak base ephedrine (Kb = 1.4 x 10-4) at 25…

A: 16.) A weak base will react with water to give hydroxide ions. So first we would write equation and…

Q: Please correct answer and don't use hand rating

A: The solutions for each question step by step. QUESTION 1:Calculate the change in pH of a 350 mL…

Q: H2SO4 + 2 NAOH 2 H20 + Na2SO4 If you require 33.35 mL of 0.541 M NaOH solution to titrate 210.1 mL…

A: The reaction occurs as follows: 2 NaOH + H2SO4 → Na2SO4 + 2 H2O 2 mol 1 mol Molarity of…

Q: = 1 0 g = 2 mol = 3 4 ☐ x10 5 An analytical chemist weighs out 0.099 g of an unknown triprotic acid…

Q: I have a question about if the Molarity of H2SO4 is good. I divide mmole with L

A: Your calculation is wrong.

Q: Sol'n MgCl soln Zine So4 Lead Nitrate Col Gre

A: " Since you have posted a question with multiple sub-parts,we will solve first three sub-parts for…

Q: fill out this table! Answering just one of the columns is good enough, thank you! Trial 1…

A: The trial 1 table is filled by using following calculation. First millimoles of NaOH to end point…

Q: When added to pure water in equal quantities, a Base with a Kb = 2.4 x 10-8 will cause greater pH…

A: when base B is added to water it abstract hydrogen ion from water to form BH+ the reaction is…

Q: Part A Calculate the solubility (in grams per 1.00 x 102 mL of solution) of magnesium hydroxide in a…

A: Solubility product for Mg(OH)2 is given by Ksp = 5.61×10−12 Part A: Given that: pH = 12 Calculate…

Q: Which of these mixtures represents a shift in the reverse direction? Select all apply

A: Here Reaction takes place in which equilibrium is established.

Q: Table 7 Measured PH 4.0 4.11 4.0 12.00 4.90 HAC Ac HAC/Ac-4.0 Calculated pH 4.0 4.14 4.0 12.00 4.0…

A: To solve this problem we need to take the calculated pH to find the experimental Ka value and the…

Q: Calculate the pH of a solution that contains 0.375 M HCN and 0.400 M NaCN Data: Ka of HCN = 6.2 x…

A: Her we have to determine pH of a solution containing 0.375M and 0.4M NaCN . The above solution is a…

Q: Question 64 W Sample pH Before Filtration Mass of Crystals 1 8.5 0.00 g 7.4 0.00 g 3 6.8 0.03 g 4…

A: The number of moles of the solute that can be dissolved per liter of solution before the solution…

Q: ↳ In the titration of HF with NaOH, which species are present at the equivalence point? HF and H₂O…

A: In this question we have to tell which species present at the equivalenc point.

Q: Question 2

A: The reaction between a weak acid, HA and NaOH takes place as follows: Calculation of no. of moles…

Q: Part 1 Raindrops found in an unpolluted atmosphere (where CO₂ (g) concentrations are 0.000390 atm)…

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

Q: What is the pH of the solution that results from mixing 25 mL of 2.60x10-2 M NH3 and 25 mL of…

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

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

Step 2

Step 3

Step 4

Step 5

Trending now

This is a popular solution!

Step by step

Solved in 5 steps

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

Timer Notes Evaluate Feedback Consider the titration of 100.0 mL of 0.8 M H₂A by 0.8 M KOH for the next three questions. The triprotic acid has Ka: 1.0 x 10-5, Kaz= 1.0 x 108, and an unknown value for Ka 1) Calculate the pH after 100.0 mL of KOH has been added. pH= Submit Answer Tries 0/45 2) Calculate the pH after 150.0 mL of KOH has been added. pH = Submit Answer Tries 0/45 3) The pH of the solution after 200.0 mL of KOH has been added is 10.00. Determine the value of Kay for this triprotic acid. Use scientific notation to enter this answer, e.g. 1.0 x 1031.00-3. Kay= Submit Answer Tries 0/45
Pre-lab question #10-1: The PH of a 0.1 M MCI (M+ is an unknown cation) was found to be 4.7. Write a net ionic equation for the hydrolysis of Mt. M* + H20 + MOH + H* M* + 2 H20 + M(OH)2 + 2H* M* + H20 + MH + OH M* + H20 → M* + OH" + H+
Which of the following salts would give you the lowest concentration of sulfate ions in solution if you placed 1 mole of the salt in a liter of water? Question 6 options: A) BaSO4 Ksp= 1.1 x 10-10 B) CaSO4 Ksp= 2.4 x 10-5 C) SrSO4 Ksp= 2.8 x 10-7 D) PbSO4 Ksp= 1.8 x 10-8
QUESTION 11 How many milliliters of 2.00 M KOH have been titrated into 35.0 mL of 0.35-M nitrous acid to obtain a solution with a pH equal to 3.57? The Ka of nitrous acid is 4.6 x 10-4. 10.24 mL 8.47 mL 5.39 ml 3.86 mL
QUESTION 5 What is the pH of a buffer system prepared by dissolving 10.70 grams of NH 4Cl and 30.00 mL of 12 M NH 3 in enough water to make 1.000 L of -5 solution? Kb = 1.80 × 10 for NH 3. %3D 9.26 9.51 11.32 9.00 Click Save and Submit to save and submit. Click Save All Answers to save all answers. Save MacBook Air DII F8 F9 F7 F6 F5 F4 F3 F2 & 24 7 3 4. 6. కాాు 00
[References] A 8.90 g sample of benzoic acid was dissolved in water to give 61.4 mL of solution. This solution was titrated with 0.360 M NaOH. What was the pH of the solution when the equivalence point was reached? K, of benzoic acid is 6.3 x 10-5. pH = Submit Answer Try Another Version 9 item attempts remaining
Please don't provide handwritten solution .....
QUESTION 8 What would be the equivalence point when 0.15M pentanoic acid is titrated with 0.1M NAOH? OA PH=7 OB. pH > 7 OC pH > 10 OD.pH <7 OE PH<3 QUESTION 9 The pkb of morphine( a weak base) is 6.1. What is the pH of a 0.077 M solution of morphine? Write answer in decimal form to the two decimal places. K, = 1.0x104 pH = pka + log[A ]/[HA] pH = -log[H,0"] 14 = pH + pOH QUESTION 10 Which of the following organic acids is the strongest
Equation: M1V1=M2V2
Question: The titration of a 25.0 mL sample of an aqueous solution containing HNO3 requires 18.6 mL of 0.150 M Ba(OH)2 to reach the equivalence point. The concentration of HNO3 in the original solution was ______ M. What I did: c=n/V n=0.150M * 18.6 mL * (10^-3 L)/1 mL = 0.00279 mol c= 0.00279 mol/25.0 mL * 1 mL/(10^-3 L) = 0.1116 M --> 0.112M It says it's wrong but I think the wording just confused me. I think I have the right idea though but I just don't know where to go with this. How can I fix my math so that I have the correct answer?
SIMULATION pH of Buffer Solutions [NH4+] = 0.10 M [NH3] = = 1.00 M H3BO3/H₂BO3 H₂CO3 / HCO3- HOCI / OCI- Check + NHÀ /NH3 HCO₂H/HCO₂ O HCO3- / CO3²- = 10.25 pH pk = 9.25 K₂ = 5.6 × 10-10 Which of the following best describes the control of buffer pH? A buffer's pH is near the weak acid's pk and shifts with changes in the [base] or [acid]. The pH of a buffer depends only on the relative concentrations of the weak acid and weak base present. The pH of a buffer depends only on the pk of the weak acid. Next> (7 of 7)
Please correct answer and don't use hand rating