Discussion:1- Why does (N22CO3) be used for HCl titration.2- Why HCl and NaOH are considered secondary standard solution?3- Is the using large quantity of indicator effect on titration?4- Why did we wash the walls of flssk during the titration?

We can determine the strength of HCl by titrating it against sodium carbonate solution using methyl…

Answered: Discussion: 1- Why does (Na2CO3) be…

Science

Chemistry

Discussion: 1- Why does (Na2CO3) be used for HCl titration.

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: Mouthwash acts to clean and disinfect mouths. Two important considerations when designing a…

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

Q: If we have a 25 mL solution of weak acid HA (Ka = 1,00 * 10-6) and at pH 4,00. How much water needs…

A: For case of dilution following formula is used M1V1 = M2V2 When m1 = Conc. of [H+] in previous…

Q: 2)[CLO-1] The aqueous solution of H;NCH;CH;NH, CI is going to be- Note that for ethylene diammonium…

Q: CHEMWORK Consider a buffered solution containing CH2NH3C1 and CH;NH,. Which of the following…

A: pOH = pKb + log salt / base Salt = CH3NH3+ Base = CH3NH2 If base is more than salt than pOH is less…

Q: Question attached

A: The midpoint of titration is the point at which excess of titrant has been added to neutralize half…

Q: 0.3872g of an unknown weak acid with general formula HY, was dissolved in water and made up to a…

A: Since HY has 1 replaceable H, it is a monoprotic acid. Equation for the association of HY is: HY(aq)…

Q: Question: The three-protic acid H3A has acid constants Ka1 = 1.00 x 10-4, Ka2 = 1.00 x %3D %3D 10-7,…

Q: Calculate [A] and [A2-]of a 0.50 M solution of diprotic acid, H₂A, with K₁ = 3.0 x 10-³ and K₂ = 5.0…

A: We will construct an ICE table and using the equilibrium constant we will calculate the…

Q: VB MB Sq What is the pH of a solution prepared by mixing 50.0 mL of a 0.10M solution of HF with 25.0…

A: Using Henderson hasselbalch equation we can calculate the pH of buffer solutions.

Q: Give typed solution A compound has two carboxyls and one aminium group. The pKas of the groups are…

A: A compound has two carboxyls and one aminium group. The pKas of the groups are 2.1, 4.5, and 9.1,…

Q: 5. Estimate the concentration of Ethanoic acid of a buffer solution containing 16.4 g/L CH3COONa and…

Q: 1. A 0.3645 sample contains only KCI and BaCl₂. This sample yielded 0.5983g of dried AgCl. Calculate…

A: Given data: Mass of the sample = 0.3645 g Mass of dried Agcl = 0.5983 g Also, the molar mass of…

Q: help please answer in text form with proper workings and explanation for each and every part and…

A: The acidity or alkalinity of a mixture is determined by its ph. The hydrogen ion (H+) concentration…

Q: 2- Calculate the hydronium ion concentration and the pH of a 10-2 M NaH2A solution. Given: The…

A: pH of salt solution of weak acid and strong base is calculated using respective formulas.

Q: The phthalic acid is a diprotic acid (pKa1-2.95, pK₂2-5.41). A titration sample was prepared by…

A: mass of phthalic acid taken = 2.23 g Molar mass of phthalic acid = 166.14 g/mol => moles of…

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

A: Given, Note: Lower the value of pH higher will be the acidity. Ranking the following solutions…

Q: Part A MISSED THIS? Read Section 18.2 (Pages 788 - 799) ; Watch KCV 18.2B, IWE 18.2. a solution that…

Q: (2). For the buffer system in Problem no. 1, what will be the pH when (a) 15.0 ml of 0.500 M HCl and…

A: since you have asked for second question, we are providing a solution for question 2 only

Q: You are titrating a 10.00 mL aliquot of a 0.3675 M solution of a diprotic weak acid (pKal = 2.125,…

A: When a diprotic acid is titrated with a strong base, two equivalence points are observed due to the…

Q: 1. a. What is the pH of a solution prepared by adding 25.0 mL of 0.10 M acetic acid (Ka ) and 20-x:…

A: 25.0 mL of 0.1 M acetic acid and 20 ml of 0.1 M sodium acetate are mixed. Acetic acid is a weak acid…

Q: The reaction HCO3 CO2+ H is an important part of the carbonate system, and is governed by the…

A: (a). pH of a solution can be defined as the negative logarithm of the value of the molar…

Q: (1). What will be the pH when 50.0 ml of 2.00M carbonic acid is mixed 20.0 ml of 3.00 M sodium…

Q: Propionic acid is provided (pKa = 2.0) to make a 0.1 M buffer at pH = 2.0. What is the ratio of…

Q: Calculate the volume, in milliliters, of a 0.530 M KOH solution that should be added to 4.750 g of…

A: Given, The mass of HEPES = 4.750 gMolar mass of HEPES = 238.306 g/molMolarity of KOH = 0.530 MpH of…

Q: 1. Based on your knowledge on pKa, pH and ionisation describe a method whereby you can separate a…

A: Ans 1. One method to separate a solution containing sodium bicarbonate and ascorbic acid is based on…

Q: Which of the following statements is true concerning a 0.50 M hydrozine N2H4 solution of 30.0 ml…

A: When there is no HCl solution, then the solution contain only N2H4 solution. By addition of HCl,…

Q: Ha Hos a. Fill in the following table using measured values: Mass or volume of A measured during lab…

Q: 1. What is the concentration of the OH- ion in 0.03 M HCl? 2. What molarity of butanoic acid (pka) =…

A: Here, HCl is a strong acid and butanoic acid is a weak acid.

Q: Be sure to answer all parts. Calculate the concentrations of H₂C₂O4, HC₂0, C₂02, and H ions in a…

A: [C2H4O2]=0.271 MKa1=6.5×10-2Ka2=6.1×10-5

Q: Consider a water sample in a closed system with Cr,c03-8x10-4 M and pH=8. a) What is the alkalinity…

A: Given, CT,CO3=8×10-4M and pH= 8

Q: 4. Explain both HCO3¯ and HSO4¯ act as amphoteric substance.

Q: In this experiment, you titrated H3PO4 with NaOH. When the titration was done, all that remained…

A: Na3PO4(aq) or PO43-(aq) is a weak triacidic base, whereas HCl is a strong acid. Hence the titration…

Q: Calculate the concentrations of H₂C₂O4, HC₂04, C₂042, and H* ions in a 0.261 M oxalic acid solution…

Q: 2-aminophenol hydrochloride is pictured at right. As is, the acid is fully protonated, the H from…

A: 2-aminophenol hydrochloride, HO-C6H4-NH3+Cl- is a diprotic acid with pka values of 4.70 and 9.97.…

Q: Calculate the pH of sodium benzanoate having a (Ka= 6.28 * 10-5) and 0.21 M sol in H2O at room…

Q: 3. Phosphonic acid, H3PO3, is a diprotic acid that can be used to prepare buffers close to…

A: Given:The phosphoric acid has the following ionizationsSince the given pH () is nearer to second…

Q: You have 0.600 L of an 0.300 M acetate buffer solution (i.e. [HC2H3O2] + [C2H3O2] = 0.300 M) at pH…

A: We are provided with 0.600 L of 0.300 M acetate buffer solution having a pH of 5.30. We are required…

Q: Ka1 = 1,11.10-2 , Ka2 = 1.11.10-7 )

A: Above solution is an acidic buffer solution, for which pH can be calculated by using Henderson…

Q: A small amount of NH4+ (pKa = 9.3) is added to a phosphate buffer at pH 7.4. Calculate the % base…

A: given: pka = 9.3 pH = 7.4 To find: % base form of ammonia at equilibrium.

Question

Discussion:
1- Why does (N22CO3) be used for HCl titration.
2- Why HCl and NaOH are considered secondary standard solution?
3- Is the using large quantity of indicator effect on titration?
4- Why did we wash the walls of flssk during the 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

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

Question 1: Calculate the pH and the equilibrium concentration of CO32- in a 7.54×10-2 M carbonic acid solution, H2CO3 (aq).For H2CO3, Ka1 = 4.2×10-7 and Ka2 = 4.8×10-11 pH=?? [CO32-] = Question 2: A 22.0 mL sample of 0.277 M trimethylamine, (CH3)3N, is titrated with 0.313 M nitric acid.At the equivalence point, the pH is ___? (CH3)3N kb=6.4x10^-5
1. For each of the solutions in part 3, calculate an expected pH. The Ka for HC₂H3O2 is: 1.8 x 10¹5 and the Kb for NH3 is 1.76 x 10. Remember to account for the dilution factor. a. 10.0mL of 0.10 M HC₂H₂O2 + 5.0mL of 0.10M HCI b. 10.0mL of 0.10M NH₂ + 5.0mL of 0.10M NaOH c. 10.0mL of 0.10M HC₂H₂O₂ +10.0mL 0.10M NaC₂H₂O₂ d. 10.0mL of 0.10 M NH3 + 10.0mL of 0.10M NH₂CI 2. Which solution(s) in question 1 would be considered a buffer solution? 3. Complete the calculation for K, from the earlier discussion of the amphoteric salt. Will this ion be acidic or basic? Predict the expected pH for the 0.050M solution. (1) H₂PO4 (aq) + H₂O → H3O*(aq) + HPO42(aq); Ka2 = 6.2 x 10-8 (2) H₂PO4 (aq) + H₂O → Kw H3PO4(aq) + OH(aq); Kb = ??? Kal 4. Similarly, the HPO4 ion is also amphoteric. The two possible reactions are: (1) HPO4² (aq) + H₂O → H3O*(aq) + PO4³(aq); Kas = 4.2 x 10-¹3 (2) HPO4 (aq) + H₂O Kw → H₂PO4 (aq) + OH(aq); Kb = <= ??? K₁2 Complete the calculation for Kb. Will this ion be acidic or…
What is [H3O+] and the pH of a solution of H2CO3 with [H2CO3]Total = 4.5 x 10-4 M? (Use the pKa value for H2CO3 given in Problem 3.) Hint: This is not a buffer.
It's not graded question... please don't reject it
please see screenshot for question and show work.
Acids and Bases Chapter 17 Non-Algorithmic Question 21 Part A You wish to prepare an HC2H3O2 buffer with a pH of 5.14. If the pKa of is 4.74, what ratio of C2H3O2 /HC2H3O2 must you use? O 0.40 O 6.0 O 2.51 O 0.40 O 0.10
Given: Concentration, Volume, Temperature (20C) Calculated: Molarity, Concentration of OH- and Ca2+ What is the information needed to know if Ksp will increase or decrease with temperature? What is the effect on Ksp when temperature is increased?
Enumeration SUBJECT: ANALYTIC CHEMISTRY
help asap A sample containing both HCl (FW 36.45) and HNO3 (FW 62.98) had a density of 1.083 g/mL. A 10.00-mL aliquot of this sample required 25.29 mL of 0.1163 M NaOH for titration. Another 10.00-mL aliquot of the sample required 20.75 mL of 0.1216 M AgNO3 for titration. Calculate the % HNO3 in the sample.
Question 5
Need help with question number 3
Only typed solution