Assigned weak acid: ,_Hydrocyanic acid (HCN)Literature K, of assigned acid:_4.9 x 10^-10Initial pH of weak acid solution:4.60_Indicator used:_PhenolphthaleinCalculated InitialConcentration of WeakAcid (M)pHvolume of NaOH (mL)Indicator endpointTitration curve|10.072211.45251equivalence pointHow to get the initial concentration of Weakacid at the Indicator endpoint? Given theconcentration fo NaOH is 1M, the initialvolume of HCN is 25ml.

Answered: Image /qna-images/answer/215ba3e5-33b6-4a93-9329-213adb4ec820.jpg

volume of NaOH (mL) Concentration of Weak Acid (M) pH Indicator endpoint Titration curve equivalence point 10.07 22 11.45 25 1 How to get the initial concentration of Weak acid at the Indicator endpoint? Given the concentration fo NaOH is 1M, the initial volume of HCN is 25ml.

volume of NaOH (mL) Concentration of Weak Acid (M) pH Indicator endpoint Titration curve equivalence point 10.07 22 11.45 25 1 How to get the initial concentration of Weak acid at the Indicator endpoint? Given the concentration fo NaOH is 1M, the initial volume of HCN is 25ml.

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: Row A. B. C. D. Use the following information to answer questions 38 and 39. A Sample Titrated with…

A: The solution is given below -

Q: Which one of the following titrations is expected to have a pH < 7 at the equivalence point? A) HNO3…

A: A solution is said to be acidic when the pH of the solution is found to be less than 7 and for a…

Q: Concentration of HCl--0.35M Volume of HCl- 24.35 mL Volume of NaOH - 36.44 mL The data above…

A: The concentration of = The volume of HCl = The volume of =

Q: -5 What The acid form of an indicator is yellow and its anion is blue. The K₂ of this indicator is…

Q: How many mL of 0.200 M KOH must be added to 17.5 mL of 0.221 M H3PO4 to reach the third equivalence…

A: Given:Concentration of KOH in molarity = 0.200 M =0.200 mol/L ( 3 significant…

Q: When 25.0 mL of 0.650 M NaOH is titrated with HCl, 37.19 mL are required to reach the endpoint. What…

Q: An air bubble of some size was present in the liquid in the buret at the end of the first titration…

A: Considering that you are titrating NaOH with some acid by taking NaOH in burette and acid in the…

Q: What is the pH of a 0.045 M solution of TRIS base? Answer:

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

Q: Given the data for the following separate titrations, calculate the molarity of the HCl: mL…

A: Recall the formula V1M1= V2M2 Where V1 is volume of NaOH M1 is molarity of NaOH…

Q: Four solutions of unknown HClHCl concentration are titrated with solutions of NaOHNaOH. The…

A: Molarity of NaOH, volume of NaOH used and volume of HCl is given we need to find the molarity of HCl…

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: What would happen to the ratio?

A: PH of a solution = - log [H+] From the relation we can say that pH of solution is inversely…

Q: A 0.12 N HNO3 solution is titrated with potassium hydroxide. 20 ml of unknown KOH solution consume…

A: The normality of a solution is the number of equivalents present in 1 liter of the solution. The…

Q: Sketch an accurate titration curve by plotting pH as a function of mL of HCl added when a 40 mL…

A: Ammonia is a weak base. Kb for ammonia is 1.8×10-5. Calculate pH of the solution when 0 mL HCl is…

Q: in acid-base titration 50.0 mL of a solution of sodium hydroxide is neutralized by exactly 12.50 mL…

A: We know that for acid base titration of H2SO4 and NaOH H2SO4 is dibasic. So, 2M1V1 = M2V2 M1 =…

Q: What volume (mL) of 0.2173M NaOH is required to titrate 50.00mL of 0.2980M HCI ?In the titration of…

A: In acid base titration same equivalent of base and acid react with each other to neutralize. The…

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

Q: Indicators can be used to help approximate the pH of a solution based on the indicator colour. Here…

Question

Assigned weak acid: ,
_Hydrocyanic acid (HCN)
Literature K, of assigned acid:
_4.9 x 10^-10
Initial pH of weak acid solution:
4.60_
Indicator used:
_Phenolphthalein
Calculated Initial
Concentration of Weak
Acid (M)
pH
volume of NaOH (mL)
Indicator endpoint
Titration curve
|10.07
22
11.45
25
1
equivalence point
How to get the initial concentration of Weak
acid at the Indicator endpoint? Given the
concentration fo NaOH is 1M, the initial
volume of HCN is 25ml.

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

Introduction

VIEW

Explanation

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 2 images

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

Explain the difference between an indicator endpoint for a titration analysis and the true equivalence point for the titration. Please simplify the answer so I can understand. Thanks
At the equivalence point, all of the acid has been neutralized by the base. Why does the pH change so sharply around the equivalence point?
Please don't provide hand written solution.....
1. Answer the following, use the data and plot as a reference, answer the following questions:a) What volume of 0.100 M NaOH solution is required to reach the equivalence point, at which the solution is completely neutralized?b) Briefly explain why the pH of the solution drastically increases once the titration proceeds past the equivalence point. c) The end point in a titration of 50.00 mL of aqueous NaOH was reached by the addition of 35.23 mL of 0.250 M aqueous HCl titrant. Calculate the molarity of the NaOH solution. The titration reaction equation is:NaOH (aq) + HCl (aq) → NaCl (aq) + H 2O (l)
If a 0.552M HCl caq) solution is used by a scientist to titrate 10.00mL of a weak base, based curve (shown below), what base? write your the titration the concentration of the auswer with 4 decitual places. pH Curve OM is 12 10 8 6 4 2 0 5:0 2 1.5 n 3 3.5 A Volume of Titrant / mL 7.5 8 8.5
A solution which is yellow in the presence of alizarin yellow indicator and red in the presence of phenolphthalein, must have a pH which is in what range? Refer to precision of indicators in the picture what is the lowest possible ph and the highest possible ph ?
From the following set of titrations choose the three most concordant titres and calculate the average titre value run 1 2 3 4 4 titre (ml) 13.40 13.70 13.85 13.45 13.80
0.2 mL of 0.10M NaOH is needed to titrate an unknown acid with a volume of 10.15mL. The final concentration of the resulting titrated sample is 0.163. Kindly explain how that value was found.
It was assumed: a) Before any acetic acid was added, essentially all the indicator was in the In- form. b) After the HCl was added, essentially all the indicator was in the HIn form. Justify these assumptions using the measured pH of these solutions and your experimental value for pKHIn to determine: 1) The fraction fo the indicator in the HIn form in solution B before any of solution A was added 2) The fraction of the indicator in the In- form after the HCl was added.
An indicator has a pk, of 7.63. In a solution with a pH of 9.35, the color in the solution will be due to which species or mix of species: O No answer text provided. O protonated indicator, Hln O indicator anion, In- O a mix of equal amounts of anion and unionized indicator