2. A0.2001g sample of Na2CO3 required 25.10ml of x's HCI to reach endpoint. The x's HCl was titrated and required 3.20ml of 0.02M NAOH soln. Calculate the molar concentration of HCI. Na2CO3 + 2HCI --> 2NACI + H20 + CO2 HCI + NAOH --> NaCl + H2O

2. A0.2001g sample of Na2CO3 required 25.10ml of x's HCI to reach endpoint. The x's HCl was titrated and required 3.20ml of 0.02M NAOH soln. Calculate the molar concentration of HCI. Na2CO3 + 2HCI --> 2NACI + H20 + CO2 HCI + NAOH --> NaCl + H2O

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: Consider the titration of 20.0mL of 0.067 M benzoic acid (C6H5COOH). a) How many mL of 0.052 M NaOH…

A: Whenver an acid and base reacts with each other than they form salt and water and the process is…

Q: Stock solution of NaCl is 0.8 M and KCl is 0.5M in concentration. Buffer Bhas 150 mM NaCl and 200 mM…

A: We need to use the dilution formula, M1V1 =M2V2 M1 is the molarity of solute in the stock solution…

Q: For each region A - F in the titration curve of a weak acid and strong base identify the generic…

A: The titration curve is for diapeotic weak acid vs strong base titration. pH of the solution depends…

Q: Given: The pH of the buffer is 4.88 made by combining 0.500 L of 0.380 M HC3H5O2 (Ka=1.30X10-5) and…

A: The Henderson Hasselbalch equation for acidic buffer is given as :

Q: 10- 8- 6- OH 2- H30¹ **** 10 strong acid strong base B A ... 20 30 40 Volume titrant (mL) Aside from…

A: Answer:Since, on adding the volume of titrant, pH of the solution is decreasing, therefore it is…

Q: 2. (a) Is it possible to measure acetic acid in the presence of HCI (each with a concentration of…

Q: In a titration of 68.0 mL of a 0.500 M solution of a diprotic acid H¿C3H;O4 (malonic acid) with…

Q: The pK, value for HF is 3.14. Would a buffer prepared from HF and NaF with a pH of 1.14 be…

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

Q: Given: The pH of the buffer is 4.88 made by combining 0.500 L of 0.380 M HC3H5O2 (Ka=1.30X10-5) and…

A: A buffer solution is formed by : 1)Mixing a weak acid with the salt solution containing its…

Q: In the titration of 50.00 mL 0.0200M weak base B using 0.0150 M HCI, which indicator is the best one…

A: Given: Weak base = 0.0200 M Volume of weak base = 50.0 mL Concentration of base = 0.0150 M pKb of…

Q: Suppose a back titration occurs that consists of 1.895grams of CaCO3 antacid (assume no buffer). The…

A: Introduction: As per the international system of unit (SI), mole is the unit of measurement for the…

Q: are the moles of base

A: Given, mass of base = 1.895g Moles of acid = 528×10-³ Volume of acid = 1057mL

Q: 1. A 15ml portion of HCl soln is reacted with 25ml of 0.01M AKOH)3 soln. to reach the end point.…

A: The number of moles is a ratio of the mass of a substance to the molar mass of the substance.…

Q: Consider the titration curves at the right. If 20mL of base was used in each titration, which…

A: The given titration curve is represented as follows:

Q: Question 5 of 7 What quantity in moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of…

A: Given -> Volume of HF = 200.0 ml = 0.209 L (1L = 1000ml) Molarity of HF = 0.200 M pH = 4.30 Ka…

Q: I need help with number 5.

Q: Calculate the pH of the solution formed when 10.0 mL of 0.15 M NaOH is added to 50.0 mL of a buffer…

Q: pre-equivalence end stage equivalence post-equivalence

A: Titrant is the substance which is added in analyte to major the pH . If we add more titrant. Then…

Q: Which of the following 1:1 mixtures would be best suited to form a buffer closest to a pH of 10 5? O…

A: SOLUTION: Step 1: The pH of a buffer solution can be calculated from the Pkb value as follows.…

Q: 7. You have 1.0 L of 100 mM K₂HPO, solution. What volume of 1.0 M HCI must be added to adjust the pH…

A: When HCl is added to K2HPO4 solution, HCl will donate it's proton. So we would first draw an ICE…

Q: 0.0 mL of 0.600 M KOH is titrated using 0.400 M H2SO4. What is volume of H2SO4 needed to reach the…

A: Answer is 30.0 ml

Q: In a titration of 32.0 mL of a 0.250 M solution of a triprotic acid H,PO, (phosphoric acid) with…

A: Given- Volume of H3PO4 =32.0 mL Concentration of H3PO4 =0.250M Concentration of NaOH=0.800 M

Q: You are given the following: 0.5 M KH2PO 4, 0.5 M K2HPO 4,0.5 M Tris base, 0.5 M Tris HCI and 3 M…

A: Interpretation: To find molecular mass of each compound given in the question and prepare the given…

Q: c) A student titrated 50.0 mL of a 0.10 M solution of a certain weak acid with NaOH. The results are…

A: Identify a pH value between 2.5 and 7.5 at which the concentration of the weak acid being titrated…

Q: Now you use the above standardization NaOH (0.0702mol/L) to titrate a 25.0mL aliquot of H2SO4. It…

A: Given, Concentration /molarity of NaOH = 0.0702 molL=0.0702 M Volume of NaOH = 12.0 mL Volume of…

Q: A student needs to prepare a buffer solution with a pH of 4.67. Assuming a pkg of 4.69, how many ml…

A: According to Henderson Hasselbalch equation, the pH of a buffer is given by, pH = pKa + log Volume…

Q: 2. A0.2001g sample of Na2CO3 required 25.10ml of x's HCl to reach endpoint. The x's HCl was titrated…

Q: The assigned buffer will be a 0.10 M, pH 6.70 buffer. The only available reagents are: 0.20 M…

A: We need to prepare the buffer with pH 6.70.

Q: In a titration of 38.0 mL of a 0.500 M solution of a diprotic acid H₂C3H₂O4 (malonic acid) with…

Q: When 10.23 ml of an unknown weak acid was titrated, it required 12.08 mL of 0.423M NaOH to reach the…

A: Given that : Volume of NaOH (V1) = 12.08 mL Molarity of NaOH (M1) = 0.423 M Volumes of weak acid…

Q: Starting with 20.0 mL of 0.126 M C6H5CO₂H (pK₂ = 4.19) and using 0.063 M NaOH as a titrant,…

A: Concentration of C6H5COOH (aq.) = 0.126 (M), Volume = 20 mL = 0.02 L Concentration of NaOH (aq.) =…

Q: nts) Consider the following buffer system, made up of E HOCI+H₂OOCI + H₂O NaOCI H₂O Na + OCI A) Is…

A: A buffer system may be if two types, one is that which consist of a weak acid with its conjugate…

Q: An analytical chemist is titrating 165.0 mL of a 0.7400M solution of methylamine (CH3NH2) with a…

A: Given,molarity of methyl amine ( CH3NH2 ) = 0.7400 MVolume of methyl amine ( CH3NH2 ) = 165.0…

Q: None

A: Step 1:To solve this problem, we can use the concept of stoichiometry and the equation of the…

Q: NH4OH pKb = 4.76. Calculate volume of 0, 1 M ammonia NH4OH and 0, 1 M ammonia chloride NH4Cl needed…

A: The objective of this question is to calculate the volume of 0.1 M ammonia and 0.1 M ammonium…

Q: For a saturated solution of an unknown metal hydroxide (M(OH)₂), 13.75 mL of this solution were…

Q: A 50.0 ml aliquot of a 0.0010OM solution of acetic acid (K = 1.8 x 10-5) is titrated with 0.00993M…

Q: Determine the mass of solid NaCH,COO that must be dissolved in an existing 500.0 mL solution of…

A: Buffer solution is the one which resists pH change on addition of small amount of acid or base in…

Q: Caitlin titrated 25.00 mL of 0.40 M formic acid with 0.25 M LIOH. What volume of lithium hydroxide…

A: Equivalence point: it can be define as the point where moles of the titrant are equal to the moles…

Q: 2. A0.2001g sample of Na2CO3 required 25.10ml of x's HCI to reach endpoint. The x's HCl was titrated…

A: Volume of NaOH = 3.20 mL = 0.00320L Concentration of NaOH = 0.02M Moles of NaOH= (0.02×0.00320)moles…

Q: A)What is the pH of a buffer prepared by adding 0.506 molmol of the weak acid HAHA to 0.507 molmol…

Q: 30.0 mL of 0.400 M KOH is titrated using 0.300 M H2SO4. What is volume of H2SO4 needed to reach the…

Q: 0.1988g of an unknown solid acid is combined with 50ml of deionized water. 15.5ml of NaOH with a 0.2…

A: Molarity of NaOH = 0.2M Volume of NaOH = 15.5mL Mass of diprotic acid = 0.1988g Volume of water =…

Concept explainers

Precipitation Titration

Precipitation analysis is used to analyze drugs, and to measure the salt content in food and beverages. It is an important concept from the examination point of view many practical questions are asked on the topic. This topic is significant in the professional exams for both undergraduate and graduate courses, especially for

Question

2. A0.2001g sample of Na2CO3 required 25.10ml of x's HCl to reach endpoint. The x's HCI was titrated and
required 3.20ml of 0.02M NAOH soln. Calculate the molar concentration of HCI.
Na2CO3 + 2HCI --> 2NACI + H2O + CO2
--> Nacl + H20
HCI + NaOH

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

Step 5

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

In a potentiometric titration of 80ug of monoprotic acid requires 15.00uL of 0.100N NaOH to reach the equivalence point. What is the acids equivalent weight?
In the titration of HF with NaOH, which species are present at the equivalence point? O HF, NAOH, and H20 only O NaF, NAOH, and H20 only O NaF, HF, and H20 only O NaF and H20 only O HF and H20 only
Give a clear handwritten answer with explanation
Be sure to answer all parts. What volumnes of 0.200 MHCOOH and 2.00 MNaOH would make 0.600 Lof a buffer with the same pH as a buffer made from 475 mL of 0.200 Mbenzoic acid and 25 mL of 2.00 M NaOH? Volume of HCOOH= LHCOOH Volume of NaOH= LNAOH
Jose titrated 40.00 mL of 0.25 M methylamine, CH3NH2, with 0.40 M HCI. CH3NH₂ Kb = 4.4 x 10-4 What volume of 0.40 M HCI is required to reach the equivalence point? Vol. HCI @ Equiv Pt Enter
I want handwritten solution....i will up vote
Part 3: pH after addition of 0.145mol HCl: Round your answer to 2 decimal places
Calculate the pH during the titration with NaOH after addition of: a) 50.00 mL of 0.1000 mol L-1 NaOH to 50.00 mL of 0.1000 mol L-1 CH3COOH (Ka= 1.75 x 10-5). b) Based on the table below, which indicator (A, B or C) is most appropriate to monitor this titration? Explain. Indicator A B C pKIndicator 3.8 9.3 5.0 Actual Transition Range (pH) 3.0 to 4.6 3.0 to 4.6 4.4 to 6.2
1 L - 1 F F D 1 F F C J 7₁ C " I F < 4:32 Question 11 of 13 A) CN and HCN B) CN- What is the primary species in solution at the halfway point in a titration of HCN with KOH? C) HCN and OH- D) OH- all? Tap here or pull up for additional resources Submit
Calculating the pH of a weak base titrated with a strong acid 0/5 Izabella An analytical chemist is titrating 165.0 mL of a 0.7400M solution of methylamine (CH3NH2) with a 0.4100M solution of HNO3. The pK of methylamine is 3.36. Calculate the pH of the base solution after the chemist has added 318.6 mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO 3 solution added. Round your answer to 2 decimal places. pH = ☐ ☑ ? 18 Ar
A solution containing 1.87 g of a diprotic acid H2C3H2O4 (malonic acid) was titrated with 45.5 mL of NaOH to reach the second equivalence point. What is the concentration of the NaOH solution? (MW malonic acid = 104.06 g/mol)
es) 1. Calculate the volume of the salt to be used in the preparation of 200 ml of the following buffer solutions. BUFFER DESIRED NUMBER pH 1 2 3 4 7.18 9.45 8.25 6.90 0.1M SOLUTIONS NaH2PO4/Na2HPO4 NH4CI/NH3 NH4CI/NH3 NaH2PO4/Na2HPO4 pka wwwwww 6.80 9.30 9.30 6.80 VOLUME OF ACID (ml) VOLUME OF SALT (ml)