H.Ws: 1- What is the influence of adding buffers on the chemical solutions? Give an example of oil and gas industry? 2- What is the difference between back and direct titration? and what are the main application of this titration in oil and gas industry?

H.Ws: 1- What is the influence of adding buffers on the chemical solutions? Give an example of oil and gas industry? 2- What is the difference between back and direct titration? and what are the main application of this titration in oil and gas industry?

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: . Solid sodium hydroxide is slowly added to 150 mL of a 0.0533 M silver acetate solution. The…

A: The question is based on the concept of solubility product Principle. it states that a weak…

Q: 18. A solid sample of a weak monoprotic acid HA is added to a solution of A to create a buffered…

A: Correct answer is (C). Statements II and III are true. HCl is required to neutralize the A-…

Q: A 30.00 ml sample of a 0.064 M weak acid solution is titrated with 0.068 M strong base. What is the…

A: Molarity of weak acid(HA) = 0.064 mol/LMolarity of base = 0.068 mol/LKa = 9.1610-6

Q: The titration curve attached was obtained from the titration of a 0.225 g sample of a solid acid…

A: From the titration curve, pH at the equivalence point is equal to 7.

Q: How many grams of solid NaF (MW = 42.0 g/mol) would have to be added to 1.0 L of 1.90 M HF solution…

A: We have to find How many grams of solid NaF (MW = 42.0 g/mol) would have to be added to 1.0 L of…

Q: You want to prepare 1.00 L of a buffer solution with a pH of 3.5. You are given an 0.45 M solution…

A: ICE table for the buffer solution of HNO2 and NaNO2 which will be produced after the addition of…

Q: Write the solubility equilibrium equation for calcium hydroxide, and write the Ksp equation. b.…

A: Ksp value is the multiplication of concentration of ions of a species. it refers the maximum…

Q: The Mohr indicator is chosen for an arbitrary titration. Which of the following statements would be…

A: Here we have to find a incorrect statement regarding the solution to be titrated-

Q: You’re mixing Ca(OH)2 in 100 mL of water and notice it is not very soluble. a. What is one way to…

A: a

Q: A buffered solution containing dissolved aniline, C, H, NH₂, and aniline hydrochloride, C,H, NH, Cl,…

Q: The concentration of Mg 2+ in seawater is 0.052 M. At what pH will 99% of the Mg 2+ be precipitated…

A: We have 0.052 M of Mg+2 , we have to predict the pH at which 99% of Mg+2 will be precipitated .

Q: 250.ml of 0.50 M CH3COOH is titrated with 0.65M NaOH. a.What is the pH of 250.ml 0.50 M CH3COOH?…

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

Q: What is the molar concentration of acetic acid? b. What is the molar concentration of the sodium…

A: Acetic acid is a weak acid and it dissociates as: CH3COOHaq⇋CH3COO-aq+H+aq The expression for Ka is:…

Q: 4) If you were to have a graph of a 23.5 mL of a weak acid (HA) is titrated with a strong base 0.20M…

A: The question is based on the titrations. we are titrating a weak acid with a strong base. we need…

Q: What is the pH at the equivalence point in the titration of a 22.4 mL sample of a 0.326 M aqueous…

A: Concentration of HF(M1) = 0.326 MConcentration of KOH(M2) = 0.484 MVolume of HF(V1) = 22.4 mL

Q: 6. 25.00 mL of 0,1588 M potassium hydroxide is titrated with 0.2004 M perchloric acid. a. Is this a…

A: Given : Volume of KOH = 25.00 ml Concentration of KOH = 0.1588 M Concentration of HClO4 = 0.2004…

Q: . The solubility of a salt A2B3 is 1.0 x 10-3 M. Calculate its solubility product. A. 1.08 x 10-13…

A: We know that the amount of a substance that will dissolve in a given amount of another substance is…

Q: A 100 mL sample of a 0.300 M solution of a weak monoprotic acid is titrated with 0.150 M KOH. After…

A: When a monoprotic weak acid is titrated with KOH. Then at certain range the solution behaves as a…

Q: A student was titrating a solution of hydrazine, H₂NNH₂, with a strong acid solution. Determine the…

A: In the given question we have to fill the BCA table of titration reaction between hydrazine and…

Q: The weak base propylamine (CH3(CH2)2NH2) has a Kb = 4.7 x10-4. It can be used in some…

A: Titration of weak base propylamine and strong acid HCl results into salt formation.

Q: A 50.0 mL sample of 0.155 M HNO₂(aq) is titrated with 0.100 M NaOH(aq). What is the pH of a solution…

A: The question is based on the titrations. we are titrating a weak acid with a strong base. we need…

Q: PH of diluted calcium hydroxide=7.01 1.) Hydronium ion concentration in dilute solution,M?…

A: The given pH of Ca(OH)2 = 7.01 Known, pH = -log[H+] pOH = -…

Q: 6. It takes 14.5 mL of 0.475 M NaOH to reach the equivalence point of a titration with 10.0 mL of a…

Q: 1. For the reaction: 2NH3(g) + CO2(g) 5 (NH2)2CO(s) + Hz0(g) AH = - 330 kJ Predict how each of the…

A: The effect of temperature, pressure, volume, amount of the substance to an equilibrium reaction is…

Q: Which one of the following is most soluble in water? a. CH3CH2CH2CH2CH2OH b. CH3OH с. Не-Clz, Kip 3D…

A: Since you have posted multiple questions, we are entitled to answer the first only.

Q: PH of diluted calcium hydroxide solution= 7.01 What is the hydronium ion concentration in dilute…

A: Interpretation- When pH of diluted calcium hydroxide solution= 7.01 then - To determine the…

Q: Calculate the pH of a 0.350 M solution of potassium phenolate, KC6H5O. Ka for phenol (CH5OH) is 1.0…

A: Since you have posted multiple questions, we will provide the solution only to the first question as…

Q: Calculate the molar solubility and solubility product of Ca(OH)2 for each trial.

A: please find the answer attached here

Q: 16.50 ml. a HBt soluton of unknown concentration requires 16.49 ml. of a 0.100 M KOH solution to…

A: One mole of HBr react one mole of KOH

Q: 5) You determined that the pH of a 0.1M solution of lactic acid, C,H,OHCOOH, is 2.9. What is the K,…

A: We need to find Ka of a weak acid using concentration and pH value.

Q: What is the molar solubility s of zinc hydroxide at 25°C? The Kap for Zn(OH)2 is 1.8 x 10-14 at…

Q: Consider the titration of 15.0 mL of 0.010 M HNO3 with 0.010 M NaOH. a. What is the total solution…

A: We have to calculate the data regarding the acid base titration.

Q: A buffer solution is composed of 1.923 g of KH,PO4 and 4.699 g of Na HPO4. (K, for dihydrogen…

A: Given that : Mass of KH2PO4=1.923 gMass of Na2HPO4=4.699 gKa for dihydrogen phsophate=6.2×10-8The…

Q: How many grams of solid NaF (MW = 42.0 g/mol) would have to be added to 1.0 L of 1.90 M HF solution…

Q: 3. Determine the volume of hydrochloric acid needed to reach the equivalence point during the…

Q: the reagent potassium phosphate tribasic trihydrate (K3PO4*3H2O) and 1.1M HCl and 1.1 M NaOH. you…

A: Given: The reagent potassium phosphate tribasic trihydrate (K3PO4*3H2O) and 1.1M HCl and 1.1 M NaOH.…

Q: Consider a 1.00 L solution which is 0.010 M CH3CO2H and 0.10 M NaCH3CO2. Ka = 1.8*10-5 a. What is…

A: This question can be solved using henderson-hesselbech equation.

Q: Kerosene is a nonpolar solvent, which solute will dissolve in it? (No explanation needed) A. C6H14…

A: Like dissolves Like. So polar solute dissolves in polar solvent and non-polar solute dissolves in…

Q: The solubility product constant of zinc hydroxide, Zn(OH)2, is 4.5 x 10-17. What would be the pH of…

A: Solubility product is defined as the product of the concentrations of the number of ions present in…

Concept explainers

Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

Question

H.Ws:
1- What is the influence of adding buffers on the chemical solutions?
Give an example of oil and gas industry?
2- What is the difference between back and direct titration? and
what are the main application of this titration in oil and gas industry?

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 2 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

A buffer solution contains 0.442 M CH3NH3Cl and 0.294 M CH3NH₂ (methylamine). Determine the pH change when 0.062 mol NaOH is added to 1.00 L of the buffer. pH after addition - pH before addition = pH change = C Submit Answer 54 $ 998 R F F4 V % 5 [References] Use the References to access important values if needed for this question. Retry Entire Group 9 more group attempts remaining T Cengage Learning Cengage Technical Support G 6 B MacBook Air S Y H & 7 ◄◄ N F7 U J * 8 ►ll F8 I M -0 9 K ►► F9 O -0 L F10 P 4) F11 Previous + Next> = Save and Exit 4))) F12 ( delete
A 0.4000 M solution of nitric acid is used to titrate 50.00 mL of 0.237 M barium hydroxide. a. What is the pH of the solution before adding any nitric acid? b. What is the pH at the half-equivalence point? c. What is the pH after the addition of 65.00 mL of nitric acid?
Consider Titration of 25 mL of .1 M CH3CO2H With .1 M NaOH. Calculate The pH After Adding The Following Volumes of NaOH: a. 0 mL b. 12.5 mL c. 20 mL d. 25 mL e. 37.5 mL I do know the correct answers, I just don't how to get to the answers. a. pH = 2.87 b. pH = 4.74 c. pH = 5.34 d. pH = 8.72 e. pOH = -log (0.0192 M) = 1.72 14 - 1.72 = 12.28 (I been having a hard time people getting the correct answer for part e, people keep getting 12.30 as the answer, but it is not. The correct answer is 12.28. I only remember how to do the last steps to get part e answer, which is 12.28, as it can be seen).
5. Consider a titration between 25.0 mL of 0.100 M sodium hydroxide, NaOH and 0.050 M hydrochloric acid, HCI. a. Determine pH of the base before titration begins. b. Find pH of the solution in flask after 10.0 mL of acid has been added. c. Calculate the volume of acid added at the equivalence point. d. Show that the pH of solution in flask is 2.23 after 60.0 mL acid has been delivered. e. Sketch the titration curve for the titration above f. Name the type of titration. g. Identify the colour change of indicator at equivalence point if phenolphthalein is used.
The following reaction represents which type of reaction? Na2SO4(aq) + BaCl2(aq)---> 2NaCl(aq) + BaSO4(s) a. Redox b. Titrationc. Neutralizationd. Displacement/Precipitation e. Dissolution
A buffer solution is composed of 1.923 g of KH,PO4 and 4.699 g of Na, HPO4. (K, for dihydrogen phosphate ion is 6.2 x 10-8.) a. What is the pH of the buffer solution? pH = b. What mass of KH;PO4 must be added to decrease the buffer solution pH by 0.10 unit from the value calculated in part a? Mass =
A buffer solution is composed of 1.324 g of KH,PO4 and 4.362 g of Naz HPO4. (K, for dihydrogen phosphate ion is 6.2 × 10-8.) a. What is the pH of the buffer solution? pH = b. What mass of KH;PO4 must be added to decrease the buffer solution pH by 0.10 unit from the value calculated in part a? Mass =
HCL Solution-- 20 mL HCl with 25.46 mL of 0.1240 M NaOH
Help please
Jj.107.
35
1. Define and describe precipitation titration? 2. How does it work? 3. How could chemical quantitative analyses be applied using this method?