5 b) Benzoic acid, HC7H5O2, is a weak monoprotic acid. A stock HC,H5O2 solutionwith unknown concentration was prepared.A 25.00 mL sample of the stock HCH5O2 solution was titrated with0.1234 M sodium hydroxide to the equivalence point, using phenolphthalein as anindicator. The titration took 20.26 mL of titrant (sodium hydroxide).(b) Write a balanced complete ionic equation for the chemical reaction that occurs inthis titration.

As we know, Acid base reation takes place. HC7H5O2(aq.) + NaOH(aq.) ----> C7H5O2Na(aq.) + H2O(l)…

Answered: nL sample of the stock HC>H;O2 solution…

nL sample of the stock HC>H;O2 solution was ti | sodium hydroxide to the equivalence point, usi The titration took 20.26 mL of titrant (sodium h ea balanced complete ionic equation for the che ion.

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: 5 Consider the following chemical equation: H₂A RbOH() Rb Ag+ H₂O A0.126 mol sample of impure…

A: We know that, At equivalence point the number of moles of H+ ions is equal to the number of moles of…

Q: Solid ammonium sulfide is slowly added to 175 mL of a 0.0484 M nickel(II) nitrate solution. The…

A: We need to find the concentration of sulfide ion required to just initiate precipitation. The…

Q: 2. When 50.0 mL of a 0.300 M AGNO; solution is added to 250.0 mL, 0.050 M of MgCl, a AgCl…

A: M

Q: A student wanted to determine the percent of NaOCI in a commercial bleaching solution. He diluted…

A: Given data, Mass of bleach = 5.0g Volume of flask = 100mL=0.1L Volume of sample = 25mL=0.025L…

Q: Resources Hint Check Ans Suppose a student needs to standardize a sodium thiosulfate, Na,S,0,,…

A: We have find out the concentration of standard sodium thiosulphate solution.

Q: Standard Sodium Chloride Weighed mass of NaCl Purity of NaCl Molar concentration of NaCl using…

A: Molar concentration of NaCl :M = (m × p)/ ( V × Mw ) where M is molarity, m is mass, p is purity,…

Q: On the reaction below, which compound can form a precipitate? Fe(NO:): + NaOH Fe(OH); + NaNO, * Mark…

A: 1st question:- First we will see the balanced general reaction as below, Balanced reaction,…

Q: 4. What is the pereentage purity of a sample of Al, (SO4)3 if a 0.5000-g sample produced a…

A: Given : Mass of Al2(SO4)3 sample = 0.5000 g And mass of BaSO4 precipitated = 1.000 g

Q: A10g sample of a substance of unknown molar mass requires 40 mL of standard solution for titration;…

A: Volume of the standard solution = 40 ml or 0.04 L Let the concentration (M) of the standard solution…

Q: A nknown concentration of 150.0 mL diprotic acid is titrated against 1.5 M NaOH. The initial burette…

A: Where n1 and n2 are the equivalency of acid and base respectively

Q: A 185.0 mL sample of 1.200 M Pb(NO₃)₂ is mixed with 99.50 mL of 1.500 M NaCl, and the PbCl₂…

A: The balanced chemical equation for the precipitation of lead (II) chloride can be written as:…

Q: 4. State the solubility of the following compounds (soluble or insoluble). If soluble, write the…

A: AlPO4 is insoluble in water because Al3+ ion and PO43 is stabalise each and form strong lattice.…

Q: of 0.1250 M H2SO4 is added to 100. mL of a solution of Pb(NO3)2, a precipitate of Pb O4 is then…

A: Given data set: 38 ml of 0.1250 M H2SO4 100 ml Pb(NO3)2 Molar mass of PbSO4 = 303 g The chemical…

Q: A 185.0 mL sample of 1.200 M Pb(NO3)2 is mixed with 80.50 mL of 1.500 M NaCl, and the PbCl,…

Q: A 20.0 mL solution of 0.200 M H;PO4 was fully titrated with 70.0 mL of a solution of calcium…

A: Given : Concentration of H3PO4 = 0.200 M Volume of H3PO4 solution = 20.0 mL And volume of calcium…

Q: An impure sample of potassium hydrogen phthalate (KHP) was titrated to determine the percent…

A: We will use stoichiometry of the reaction to get the answer.

Q: Solid sodium carbonate is slowly added to 75.0 mL of a 0.173 M cobalt(II) nitrate solution until the…

A: CoCO3 is a insoluble salt, when sodium carbonate add with cobalt nitrate, cobalt carbonate…

Q: had taken place. What is 3) What is the effect on the determination of the sodium hydroxide…

A: We have find out the answer. Note ~ Since you have posted multiple questions, we will provide the…

Q: Calculate the % w/w Cl– (35.45 g/mol) in the sample. Provide your answer to 2 places after the…

Q: A given 5.0 g impure sample of sodium carbonate was titrated via 0.1500 N HCl. The sample utilized…

A: Given-> Weight of sample = 5.0 gm Normality of HCl = 0.1500 N Volume of HCl = 31.55 ml = 0.03155…

Q: 100. mL of 0.10 M CaCl, is mixed with 50.0 mL of a 0.10 M solution of either Al,(SO,), Na,SO, or…

Q: 100.0 mL of a 0.245 M solution of HCl was added to 50.0 mL of 0.365 M Ba(OH)2. Answer the following.…

A: Given that: volume of HCl = 100.0 mL = 0.10 L molarity of HCl = 0.245 M volume of Ba(OH)2 = 50.0…

Q: 0.300 g of a nitrogen-containing sample is analyzed by the Kjeldahl method and the released ammonia…

A: The Kjeldahl method is a method for the quantitative determination of nitrogen contained in organic…

Q: Enter your answer in the provided box. A sample of 0.8360 g of an unknown compound containing barium…

A: Mass of baso4 ppt=0.7737g Total mass of compound= 0.8360g

Q: A solution of HCl is prepared for titration of unknown Na2CO3 samples, by standardization with pure…

A: Mass of Na2CO3 = 0.4453 g Molar mass of Na2CO3 = 105.99 g/mole Mole of Na2CO3 =…

Q: What mass of NaCl is needed to precipitate all the silver ions from 20.0 mL of 0.100 M AgNO3…

A: We know the reaction, Ag+ + Cl- ---------> AgCl AgCl is precipitated product. One mole of Ag+…

Q: Part C An impure sample of table salt that weighed 0.8571 g when dissolved in water and treated with…

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

Q: Solid cobalt(II) nitrate is slowly added to 150 mL of a 0.0512 M sodium carbonate solution. The…

A: Recall the probable reaction which will occur on addition of solid cobaltIInitrate in sodium…

Q: A 0.4574 g sample containing only NaCN and KCN requires 41.65 ml of 0.1056 M AgNO3 for titration.…

Q: 9. What is meant by a "dilute weak base?" Provide an example.

A: "Dilute weak base" is the weak base that is diluted with water .

Q: A 25.5 mL aliquot of HCl (aq) of unknown concentration was titrated with 0.113 M NaOH (aq). It took…

A: Volume of HCl (V2) = 25.5 mL Molarity of NaoH(M1) = 0.113 M Volume of NaOH (V1)…

Q: [Review Topics] [References] Use the References to access important values if needed for this…

Q: Solid potassium sulfide is slowly added to 50.0 mL of a 0.0321 M silver nitrate solution. The…

Q: A 0.5152 g solid sample containing a mixture of LaCl, (molar mass = 245.26 g/mol) and Ce(NO,),…

Q: A 0.574-g sample of a chlorocarbon compound was analyzed by burning it in oxygen and collecting the…

A: Given data: Molarity of AgNO3 = 0.28 M Volume of AgNO3 = 26.21 mL Molarity of KSCN = 0.122 M Volume…

Q: A 0.5086 g solid sample containing a mixture of LaCl, (molar mass = 245.26 g/mol) and Ce(NO,),…

A: Precipitation reactions: These are the example of double displacement reaction. In these reactions,…

Q: 1.) A sample containing 0.175 g of Cl- is dissolved in 50 mL of deionized H20. The solution is…

A: Let us solve.

Q: 0.753-g sample of a chlorocarbon compound was analyzed by burning it in oxygen and collecting the…

A: Answer:- This question is answered by using the simple concept of stoichiometry which involves the…

Q: a 1.42 g sample of pure copmound, with fornula M2SO4, was dissolved in water and treated with an…

A: The number of moles of a substance is the ratio of its given mass by molar mass of the substance. It…

Q: mL of a bleach (NaOCl) sample is diluted to 500 mL. An excessive amount of KI is added to the 20 mL…

A: The question makes use of iodometric titrations in which indirectly liberated iodine is titrated…

Q: Determine the pH at the equivalence point of a titration of 100.0 mL of 0.265 M CH₂NH₂ solution with…

A: Answer: Conjugate acid of weak base gets hydrolyzed in water and produces H3O+ ion and as CH3NH2 is…

Q: Solid sodium hydroxide is slowly added to 75.0 mL of a 0.168 M copper(II) acetate solution until the…

A: Concentration of copper (II) acetate solution = 0.168 M concentration of hydroxide ion = 0.0498 M.…

Q: 3. In a solution containing H3O* ions at a concentration of 0.003 mol.L', what is the concentration…

A: Given, [H3O+] = 0.003 mol.L-1 [OH-] = ? The formula used here are, pH = -log[H3O+] pH + pOH = 14 pOH…

Q: Phosphate in a solution is titrated with 0.08141 M solution of silver nitrate (AgNO3) as follows:PO…

A: We will calculate the moles of PO43- that can be titrated using the given mass of silver nitrate.…

Q: 18.0 g of zinc is added to 100. mL of 0.200M HBr. a) Will all of the zinc dissolve? b) What will be…

A: Given : Mass of Zn = 18.0 g Volume of HBr solution = 100 mL = 0.100 L…

Question

5 b) Benzoic acid, HC7H5O2, is a weak monoprotic acid. A stock HC,H5O2 solution
with unknown concentration was prepared.
A 25.00 mL sample of the stock HCH5O2 solution was titrated with
0.1234 M sodium hydroxide to the equivalence point, using phenolphthalein as an
indicator. The titration took 20.26 mL of titrant (sodium hydroxide).
(b) Write a balanced complete ionic equation for the chemical reaction that occurs in
this titration.

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

SEE SOLUTION Check out a sample Q&A here

Similar questions

a Pb(NO;)2 + MgSO, The precipitate is Cu(NO3)2 + ZnBr2 The precipitate is Submit (NH4)2 CO3 + Bal, The precipitate is K2 CrO4 + Pb(NO3)2 The precipitate is
Please provide the step-by-step and answer in the conversion format under the question and equation to help me better understand. Full depth on the process please ?
biloz erti lo 1) An experimenter performed a titration of an unknown weak base to fo determine the identity of the weak base, The experimenter dissolved 0.175 g of the base into 25.0 mL of deionized water, and the titrant they used was HBr at a concentration of 0.150 M. Using the table below, determine noit the Kb and the molar mass of the weak base. Iorw Volume of HBr pH 0 mL 11.96 13.0 mL 10.75 26.0 mL 5.90 30.0 mL 1.96
25.0 mL of a 0.2450 M NH,CI solution is added to 55.5 mL of 0.1655 M FeCl,. What is the concentration of chloride ion in the final solution? Select one: a. 0.607 M b. 0.276 M с. 1.35 М d. 0.418 M e. 0.190 М
1. A solution of HCIO, was standardized by dissolving 0.3745 g of primary standard grade HgO in the solution of KBr. The liberated OH required 37.79 mL of the acid to be neutralized. Calculate the molarity of HCIO.. HgOs) + 4Br + H,0 > HgBr. + 20H
What mass of Fe(OH)3 will be obtained when 100. mL of 0.240 M FeClz is mixed with 200. mL of 0.182 MNAOH? |g Fe(OH)3
A 25.0 mL aliquot of HCl (aq) of unknown concentration was titrated with 0.105 M NaOH (aq). It took 68.8 mL of the base to reach the endpoint of the titration. The concentration (M) of the acid was ________.
2.00 mL of 0.200 M Fe(NO3)3 were mixed with 3.00 mL of 0.152 M NaSCN and 3.00 mL of HNO3. The initial concentration of SCN- ions (assuming no reaction occurred) was:
Part 1 Solution A is a 5.0 L aqueous sodium iodide (Nal) solution, and I want to determine the concentration of iodide ions, I- (aq). I'm going to do this with a precipitation titration, taking advantage of the insolubility of Agl (s). To a 20.0 mL sample of Solution A, I add 0.0740 M AgNO3 aqueous solution until adding AgNO3 no longer causes more precipitate to form. I see no more visible precipitate after adding 6.00 mL of AgNO3 solution. Based on this information, what is the concentration (in mM) of iodide anions in Solution A? Part 2 mM I It's hard to precisely measure the endpoint for a precipitation titration. Let's suppose that instead of measuring the volume of AgNO3 solution added, I just measure the weight of precipitate from the above experiment. I determine that the precipitate weighs 93.9 mg. Based on the weight of the solid precipitate, what is the concentration (in mM) of iodide anions in Solution A? mM I
A sample weighing 9 g of BaCl2 is dissolved in 700 mL of water, when 50 mL of the sample is titrated with 30 mL of 0.5 N AgNO3 the percentage of chloride Cl- (A.wt = 35.5) in the sample is *
Pls ans both
An acid-base titration reaches its end point when iõð mlL of 8.2 M HCI Is ådded to 50 mL of NaOH. What is the concentration of the NaOH (M)?