A 10-ml water sample containing only C* and H" has a pH value of 3. The sample was passed through a cation exchanger H-form. ThepH of the collected solution was 2.8. Calculate the concentration of C* in the sariple.O a. 0.0048Please explain thesolution in detail.O b. 0.0006O G. 0.0002O d. 0.0005

A 10-ml water sample containing ony C* and H has a pH value of 3. The sample was passed through a cation exchanger H-form. Th pH of the collected solution was 28. Calculate the concentration of C* in the sarmple. ০ ३, 0.0048 Please explain the solution in detail. O b. 0.0006 O c. 0.0002 d. 0.0005

A 10-ml water sample containing ony C* and H has a pH value of 3. The sample was passed through a cation exchanger H-form. Th pH of the collected solution was 28. Calculate the concentration of C* in the sarmple. ০ ३, 0.0048 Please explain the solution in detail. O b. 0.0006 O c. 0.0002 d. 0.0005

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter16: Applications Of Neutralization Titrations

Section: Chapter Questions

Problem 16.30QAP

See similar textbooks

Related questions

Q: 23 (Cl) calculate the PH ot a butter Solution Conteuminy 3 mmol (NHy CL) and 3mmol (N what will the…

A: Given : Moles of NH3 taken = 3 mmol = 0.003 mol (since 1…

Q: pH of bleach I

Q: Consider a solution of 0.00200 M HCIO, for numbers 22-24. Determine the following 22. equilibrium…

A: HClO4 is strong acid hence it dissociated completely in solution

Q: Explain why the pH of mixture C is the same as the pH of mixture A. Mixtures Conductvity (mA) pH A.…

A: Here we have to explain why the pH of mixture C is the same as the pH of mixture A-

Q: is solution is prepared by mixing 25 mL of 0.1 M HCHO2 with 25 mL of .2 M NaCHO2. The pH of the…

A: Given values-> Volume of HCHO2 = 25ml Molarity of HCHO2 = 0.1 M Volume of NaCHO2 = 25 ml Molarity…

Q: LObserving pH Changes in Water and Buffer Solutions upon Addition of HCl and NaOH Seluiana solution…

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

Q: Determine the pH at the point in the titration of 40.0 mL of 0.200 M H2NNH2 with 0.100 M HNO3 after…

A: Henderson's equations enable the calculation of the pH of buffer solutions prepared by mixing known…

Q: 1- Calculate the pH of 2 solution prepared by adding 25 ml of 0.1IM of NAOH solu. to 30 ml of 0.2M…

A: 1. Millimoles of NaOH = M x V = 0.10 x 25 = 2.5 mmol Millimoles of Acetic acid = M x V = 0.20 x 30…

Q: Calculate the mass of solid NaCH3CO0 that must be added to 1.0 liter of 0.20 M CH3COOH solution so…

Q: 4. A pH buffer solution contains 1.383 mole CH3COOH and 1.875 mole CH3COONa. The volume of the pH…

Q: Samples of an unknown solution are tested with different indicators. Base on the following evidence,…

A: The pH indicator or acid-base indicators are used to determine acidity and basicity of the solution.…

Q: o) 10 ml, 0-M HCL is udded to j00 ml of asal.tron which is 0.1M both in HOAC and Na OAC. 8y how many…

Q: 73. A student dissolves 0.0100 mole of an unknown weak base in 100.0 mL water and titrates the…

A: First determine the mole of HNO3 present in 40mL of solution. The excess base present after…

Q: Which of the following pairs of substances can be used to make a buffer solution? O a. NH3 &…

A: A buffer is a solution which resist any change in pH on adding a small amount of acid or base . it…

Q: How many moles of sodium acetate should be added to 0.40 mol CH3COOH to make a solution buffering at…

A: Given- Moles of CH3COOH = 0.40 mol pH = 4.46 pKa = 4.76

Q: calculate the pH of the equivalence point N2OH soluhon Concentrahun.of n =0.lmol/L Mean titre (MOOH…

A: A titration is an analytical method that is used to determine the unknown quantity of the analyte…

Q: The table shows respective color change when a universal indicator is added to the clear solutions.…

A: Solution : Universal indicator is prepared by mixing the different indicators that show…

Q: 40.00 mL of 0.09M NaOH is diluted to 100 mL and titrated with 0.1M HCl. Calculate the pH after the…

Q: If carbonic acid (H₂CO₃) is titrated against a strong base, how many end point to we expect? a. 1…

A: Weak acid- an acid dissociate slowly into its ions in an aqueous solution to give H+ ions e.g.…

Q: A 10-ml water sample containing only Cr* and H has a pH value of 3. The sample was passed through a…

A: Hydrogen ion concentration is an important parameter of an aqueous solution. The concentration of…

Q: A solution is made by mixing 0.400M in formic acid, HCOOH, and 1.00M in sodium formate, HCOONa?…

Q: 32. A 50.00 mL of 0.0275 M HCl solution was titrated with 0.1500 M NaOH. Calculate the pH of the…

Q: 14. Calculate and compare [H₂O"] and pH for a 0.10 M solution of HCI (a strong acid) and a 0.10 M…

A: Acid are compound which releases hydronium ion when dissolve in water We are required to compare…

Q: 4. 250.0 mL. The acid dissociation constant of CH3COOH is 1.799x10-5. Please answer the following…

A: A buffer is a solution which resist any change in pH on adding a small amount of acid or base . it…

Q: IP wc dissolve an a cid weak HzA in wate, the solution volume willbe looml, and its pH=27 if you…

A: The question is based on the concept of chemical equilibrium. We have to calculate mass of the acid…

Q: 31. Select the BEST statement regarding a buffer solution from the following. *

A: Buffer solutions: Buffer solution is actually a mixture of weak acid and its salt with strong base…

Q: A volume of 25.0 mL of 2.75 M HCl, is to be titrated with 1.025 M strong base, B(OH)2. Calculate the…

A: The strength of an acid solution is determined by titrating it against a standard base solution or…

Q: You add 100.0 mL of 0.10 M KOH to 50.0 mL of 0.20 M HCIO. What is the pH of the resulting solution?…

A: Given: 100mL of 0.10M KOH 50mL of 0.20M HClO

Q: 35. A 50.00 mL of 0.0275 M HCl solution was titrated with 0.1500 M NaOH. Calculate the pH of the…

Q: 40.00 mL of 0.09M NaOH is diluted to 100 mL and titrated with 0.1M HCl. Calculate the pH after the…

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…

Q: Determine the pH at the point in the titration of 40.0 mL of 0.200 M H2NNH2 with 0.100 M HNO: after…

Q: Consider a solution that has 0.00500 M HCl and 0.100 M HF. Ka of HF = 7.2x10-4. a. What is the pH of…

A: Given:Solution : 0.00500 M HCl and 0.100 M HFTo determine:(a) pH of the solution.(b) pH of the…

Q: 3. Why is casein plastic no longer used in large-scalę manufacturing?

A: Answer- casein is used to make plastics today that are used for items like fountain pens. It was…

Q: 38. Determine the pH of 0.42 M for formic acid, HCOOH solution. The value of pka for HCOOH is 3.75.…

A: We have to calculate the pH of Solution.

Q: Calculate the pH in the titration of 25 mL of 0.10 M HCl by sodium hydroxide after the addition to…

A: Welcome to bartleby !

Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

A 10-ml water sample containing only C* and H" has a pH value of 3. The sample was passed through a cation exchanger H-form. The
pH of the collected solution was 2.8. Calculate the concentration of C* in the sariple.
O a. 0.0048
Please explain the
solution in detail.
O b. 0.0006
O G. 0.0002
O d. 0.0005

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

Step 2

Step 3

Step 4

Final answer

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

A 0.3012g sample of an unknown monoprotic acid requires 24.13mL of 0.0944MNaOH for neutralization to a phenolphthalein end point. There are 0.32mL of 0.0997MHCl used for back titration. a. How many moles of OH are used? How many moles of H+ from HCl? _______moles OH ________moles H+ b. How many moles of H+ are there in the solid acid? Use Eq.5. ____________ moles H+ in solid c. What is the molar mass of the unknown acid? Use Eq.4. ____________ g/mol
. How is the strength of an acid related to the fact that a competition for protons exists in aqueous solution between water molecules and the anion of the acid?
A diprotic acid, H2B(MM=126g/moL), is determined to be a hydrate, H2B xH2O. A 10.00-g sample of this hydrate is dissolved in enough water to make 150.0 mL of solution. Twenty-five milliliters of this solution requires 48.5 mL of 0.425 M NaOH to reach the equivalence point. What is x?
Phenolphthalein is a commonly used indicator that is colorless in the acidic form (pH 8.3) and pink in the base form (pH 10.0). It is a weak acid with a pKa of 8.7. What fraction is in the acid form when the acid color is apparent? What fraction is in the base form when the base color is apparent?
Isocyanic acid (HNCO) can be prepared by heating sodium cyanate in the presence of solid oxalic acid according to the equation 2NaOCN(s)+H2C2O4(s)2HNCO(l)+Na2C2O4(s) Upon isolating pure HNCO(l), an aqueous solution of HNCO can be prepared by dissolving the liquid HNCO in water. What is the pH of a l00.-mL solution of HNCO prepared from the reaction of 10.0 g each of NaOCN and H2C2O4, assuming all of the HNCO produced is dissolved in solution? (Ka of HNCO = 1.2 l04.)
Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH, stoichiometric points occur at pH = 3.9 and 8.8. A 25.00-mL sample of malonic acid of unknown concentration is titrated with 0.0984 M NaOH, requiring 31.50 mL of the NaOH solution to reach the phenolphthalein end point. Calculate the concentration of the initial malonic acid solution. (Sec Exercise 113.)
Consider the following acids and bases: HCO2H Ka = 1.8 104 HOBr Ka = 2.0 109 (C2H5)2NH Kb = 1.3 103 HONH2 Kb = 1.1 108 Choose substances from the following list that would be the best choice to prepare a pH = 9.0 buffer solution. a. HCO2H b. HOBr c. KHCO2 d. HONH3NO3 e. (C2H5)2NH f. (C2H5)2NH2Cl g. HONH2 h. NaOBr
A 10-ml water sample containing only Cr* and H* has a pH value of 3. The sample was passed through a cation exchanger H-form. The pH of the collected solution was 2.8. Calculate the concentration of Cr* in the sarriple. O a. 0.0048 Please explain the solution in detail. O b. 0.0006 O c. 0.0002 O d. 0.0005
urgent one hour please
O File C/Users/yanal/OneDrive/Desktop/20105%clyaJI20%J20% Jislá 20%Glgis.pdf 00 Q EI D Page view A Read aloud V Draw V Highlight 2Erase O Bu 6d Tie man chem 105 exam form a 1 of 4 If the heat of neutralization for NAOH (1 mal) and H,SO, solution (0 6 mol) is studied and found to release Q (KJ) then the heat of neutralization (ignoring the heat absorbed by calorimeter) that in released from this solution in KJ/mol will be equal to 0005 0 006 C-003 Next Question > Assessment Navigator Forreton enteto Yarmeuk Unversty D4 ING here to search
ka = 1.8 x 10^-5
5) pH Calculations of Polyprotic Systems a. What is the pH of 0.1000 M H;PO,? (K,1 = 6.9x10) b. What is the pH of 0.1000 M NaH,PO,? (K31 = 6.9x103, K2=6.2x10*) c. What is the pH of 0.1000 M Na;HPO,? (K=6.2x108, Kg3=4.8x1013) d. What is the pH of 0.1000 M Na;PO,? (K33=4.8x10-13)