Answered: 50 ml HCl solution requires 25.5 ml,…

Science

Chemistry

50 ml HCl solution requires 25.5 ml, 0.015 M Ca(OH)2 for the endpoint with a basic indicator. What is the HCl molarity?

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Chapter16: Acids And Bases

Section: Chapter Questions

Problem 8STP

See similar textbooks

Related questions

Q: In a titration experiment a 25.0 mL sample of a diprotic acid required 30.0 mL of 0.200 M NaOH for…

Q: I need 30 mL of a buffer solution with a volume ratio of 6:1 acid:base. How do I calculate how much…

A: Given, Volume of buffer = 30mL volume ratio of acid:base = 6:1 Buffer solution: It consists of…

Q: illustrates a typical neutralization titration, one between an HCl solution of unknown concentration…

A: Solution: Here we have HCl with unknown concetration and a standard NaOH . therefore, HCl will be…

Q: What is an acid–base indicator? Define the equivalence (stoichiometric) point and the end point of a…

A: An acid-base indicator is either a weak acid or weak base that exhibits a colour change as the…

Q: For a weak acid (CH3COOH) that is titrated with a strong base (NaOH), what species (ions/ molecules)…

A: The stoichiometric point is also known as the equivalence point. It is the point when the complete…

Q: 1. Ba(OH)2 to reach an endpoint with bromocresol green indicator. Calculate the molar concentration…

A: The molarity of a solution is an important method to determine the concentration of a solution. It…

Q: Malic acid (C4H5O5) is one of the alpha hydroxy acids which is naturally found in apples. The…

A: Given data, Concentration of HCl = 7.29 x…

Q: 2.1 The correct indicator was added to 25.00 mL of a 0.1340 M solution of pentanoic acid…

A: Pentanoic acid is a weak organic acid. Its Ka is 1.4 x 10-5. Its concentration is 0.1340 M and…

Q: A 22.00 mL sample of HCl is titrated to phenolphthalein end point with 24.63 mL of a 0.08481 M NaOH…

A: Given :- Molar concentration of NaOH = 0.08481 M Volume of NaOH used = 24.63 mL Volume of HCl…

Q: A Ringer's solution consists of 140mEq/L Na+, 5mEq/L K+, 4mEq/L Ca2+, and Cl- as the only counter…

A: Given Concentration of Na+ =140 MEq/L Concentration of K+ = 5 mEq/L Concentration of Ca2+ = 4…

Q: A 25.00-mL sample of an HNO3 solution is titrated with 0.102 M NaOH. The titration requires 28.52 mL…

A: The acid base reaction is HNO3 + NaOH -------> NaNO3 + H2O Equivalent moles of acid and base…

Q: What is the molarity of an Acetic Acid solution if 25.50 mL require 25.24 mL of 0.112M NaOH to…

A: The balanced reaction between Acetic acid and NaOH is as follows:

Q: The distribution of a pH indicator that is an acid (i.e. Hln) depends on the pH of the solution that…

A: Answer is in step 2

Q: A 25.00 mL sample of 0.1000 CH3COOH is titrated with a 0.1000 M NAOH solution. Calculate the pH…

Q: Phosphoric acid is often found in soft drinks. How many mL of 0.100 M sodium hydroxide would be…

A: According to the mole concept, in terms of mass, the amount of substance in moles is equal to the…

Q: 100 mL of a natural water sample, whose pH is 6,6, requires 12,2 mL of 0,10 M HCl to end point…

Q: A 150.00 mL volume of HCI solution required 29.71 mL of 0.01963 M NAOH to reach an end point with…

Q: A buffer solution contains 0.427 mol of carbonic acid and 0.512 mol of sodium hydrogen carbonate in…

Q: In a titration of 71.0 mL of a 0.750 M solution of a triprotic acid H,C H,O, (citric acid) with…

A: The solution is given below -

Q: A mixture is made by combining 110 mL of 0.015 M HCl and 215 mL of 0.025 M HI. What is the pH…

Q: A chemistry graduate student is given 100. mL. of a 0.60M trimethylamine (CH, N: solution.…

Q: A sample of 27.0 mL of 0.310 M NAOH is titrated with 0.740 M H2SO4. How many milliliters of H2SO4…

A: Given : concentration of NaOH = 0.310 M volume of NaOH solution = 27 mL concentration of H2SO4 =…

Q: The beaker contains 0.1 M acetic acid solution with methyl orange as an indicator. Another beaker on…

A: A buffer is formed when a weak acid is mixed with its conjugate base or weak base with its conjugate…

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: What is the pH of a solution prepared by mixing 500 mL of 1.5 M HF with 400mL of 1.00 M NaF? The Ka…

Q: You want to prepare a buffer solution with pH equal to 3. How many grams of NaF (41.99 g/mol) should…

A: In this, we need to find oute moles of NaF first. Using that moles and molar mass for NaF, calculate…

Q: A 40.0 mL sample of a 0.08 M HCl solution is titrated with a 0.10 M NaOH. What volume of tiltrant is…

Q: 2) The indicator Haln has Ka = 4.5 x 105, Kaz = 4.5 x 10°. H,ln is red, HIn' is blue, In2 is yellow.…

A: Given data:-

Q: A certain indicator, HA, has a K, value of 1.0 × 10-5. The protonated form of the indicator is red…

A: pKa = -log Ka pH = -log[H+]

Q: [4} What is the pH of the solution in the flask after 25.00 mL of 0.110 M NAOH has been added to…

Q: An aqueous solution contains 0.345 M dimethylamine ((CH3)2NH). How many mL of 0.370 M hydroiodic…

Q: A 50.00-mL portion of an HCl solution required 29.71 mL of 0.01963 M Ba(OH)2 to reach an end point…

A: The number of moles of OH-, nOH-, in 29.71 mL of 0.01963 M Ba(OH)2 is; 1000 mL=1.0 LnBa(OH)2=0.01963…

Q: 50.00 mL of an acetic acid solution is titrated with 0.1000 M NaOH. 23.90 mL NaOH is required to…

A: Given : Volume of acetic acid = 50 ml Volume of NaOH = 23.90 ml Molarity of NaOH = 0.1000M

Q: 2. The ionization constant for acetic acid is 1.8 x 10-5. How many grams of NaC2H3O2 must be added…

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

Q: An aqueous solution contains 0.329 M methylamine (CH3NH2). How many mL of 0.305 M perchloric acid…

Q: The beaker contains 0.1 M acetic acid solution with methyl orange as an indicator. Another beaker…

A: A buffer is formed when a weak acid is mixed with its conjugate base or weak base with its conjugate…

Q: A 250.0 mL of 0.35 M HCl is mixed with 150.0 mL of 0.50 M NaOH. What is the net ionic equation and…

A: Applying concept of pH PH= -log [H+]

Q: It took 32.47 mL of 0.1424 M NaOH to reach the endpoint when titrating a sample containing 0.615g of…

Q: Determine the concentration of CH3COOH in a 40 mL solution if it takes 25 mL of a 0.035 M NaOH…

A: Acetic acid is a weak monoprotic acid and NaOH is monoprotic base so they reacts with each other in…

Q: It is required to prepare 100ml of a solution with pH 10 by mixing concentration ammonia (14.8M) and…

A: A solution will be a buffer solution if it is formed by the weak acid and its conjugate base or weak…

Q: I mix 100 mL of 0.100 M HCl in 250 mL of 0.150 M NH3. I add 50.0 mL of 0.0500 M NaOH. What…

Q: A 20.00 mL of 0.100 M diprotic weak acid H2A is titrated with 0.200 M NaOH. The volume of the NaOH…

Q: For 530.0 mL of a buffer solution that is 0.145 M in HC2H3O2 and 0.130 M in NaC2H3O2, calculate the…

A: Ethanoic acid is a weak acid and dissociates as:

Q: At what condition is it best to titrate with KMNO4 without using an indicator? O strongly basic…

Q: A certain indicator, HA, has a K value of 0.00032. The protonated form of the indicator is blue and…

Q: The K, for NH3 is 1.8 x 10-° at 25°C. Calculate the pH of a buffer solution made by mixing 45.7 mL…

A: Given data:- A buffer solution made by mixing 65.1 mL of 0.142 M NH3 with 38.0 mL of 0.172 M NH4Cl…

Q: The indicator methyl red has a pKHIn = 4.95. It changes from red to yellow over the pH range from…

Q: A titration of 25.00 mL of sulfuric acid required 37.22 mL of 0.1124 M NaOH to reach the endpoint.…

A: Given; The molarity of NaOH, (M1) = 0.1124 M. The volume of NaOH, (V1) = 37.22 mL. The volume of…

Q: If 0.654 g of a primary standard acid (potassium hydrogen phthalate, molar mass = 204.23 g/mol)…

A: Given data :

Q: Titration of 10.00 mL of a 0.444M solution of HCl with a solution of LiSH required 23.2 mL of the…

Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

50 ml HCl solution requires 25.5 ml, 0.015
M Ca(OH)2 for the endpoint with a basic indicator. What is the HCl molarity?
b) Describe the primer standart properties?

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 by step

Solved in 4 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 solution is made by diluting 25.0 mL of concentrated HCl (37% by weight; density = 1.19 g/mL) to exactly 500 mL. Calculate the pH of the resulting solution.
In an acid-base titration, 21.16 mL of an NaOH solution are needed to neutralize 20.04 mL of a 0.0997 M HCl solution. To find the molarity of the NaOH solution, we can use the following procedure: First note the value of MH in the HCl solution. ____________M Find MOH- in the NaOH solution. Use Eq.3. ____________M Obtain MNaOH from MOH. ____________M
What is an acidbase indicator? Define the equivalence (stoichiometric) point and the end point of a titration. Why should you choose an indicator so that the two points coincide? Do the pH values of the two points have to be within 0.01 pH unit of each other? Explain.
A bottle of concentrated hydroiodic acid is 57% HI by weight and has a density of 1.70 g/mL. A solution of this strong and corrosive acid is made by adding exactly 10.0 mL to some water and diluting to 250.0 mL. If the information on the label is correct, what volume of 0.988 M NaOH is needed to neutralize the HI solution? Suggest an indicator for the titration.
The species called glacial acetic acid is 98% acetic acid by mass (d=1.0542g/mL). What volume of glacial acetic acid must be added to 100.0 mL of 1.25 M NaOH to give a buffer with a pH of 4.20?
Ammonia gas is bubbled into 275 mL of water to make an aqueous solution of ammonia. To prepare a buffer with a pH of 9.56, 15.0 g of NH4Cl are added. How many liters of NH3; at 25C and 0.981 atm should be used to prepare the buffer? Assume no volume changes and ignore the vapor pressure of water.
A 0.400-M solution of ammonia was titrated with hydrochloric acid to the equivalence point, where the total volume was 1.50 times the original volume. At what pH does the equivalence point occur?
When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
What mass of NH4Cl must be added to 0.750 L of a 0.100-M solution of NH3 to give a buffer solution with a pH of 9.26? (Him: Assume a negligible change in volume as the solid is added.)