1. A 40.00 mL sample of 0.250 MKOH is titrated with 0.200 MHI using phenol red as the indicator (pH range 6.4-8.2). Calculate the pH for the following points in the titration. Hint: first calculate the mol of KOH remaining Total L of HI added 0.00 0.0250 0.0500 0.1000 mol of HI added 0.00 mol of OH- remaining mol of excess H+ [OH-]remaining, M [H+] excess, M pH POH

1. A 40.00 mL sample of 0.250 MKOH is titrated with 0.200 MHI using phenol red as the indicator (pH range 6.4-8.2). Calculate the pH for the following points in the titration. Hint: first calculate the mol of KOH remaining Total L of HI added 0.00 0.0250 0.0500 0.1000 mol of HI added 0.00 mol of OH- remaining mol of excess H+ [OH-]remaining, M [H+] excess, M pH POH

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: Titration Curves. Solve the ff. Problems 1. A 25mL aliquot of 0.1M NaOH is titrated with 0.10M HCl.…

Q: During the titration, how would your experimental molarity of NaOH differ from the actual molarity…

A: Please have a look on the solution:

Q: 1. A 50 mL of 0.005 M HCl sample is titrated with 0.010 M NaOH. Find the pH of the solution at…

A: HCl is a strong monoprotic acid. NaOH is a strong monoacidic base The balanced neutralization…

Q: You are required to prepare 1 litre of 0.1 acetate buffer solution having a ph of 3.5. Calculate the…

A: Buffer solution The solution that resists any change in the pH value is known as buffer solution.…

Q: . calculate the pH of the solution when an additional 5.0 mL of potassium hydroxide has been added;…

A: The question is based on the concept of titrations. we are titrating a weak acid with a strong base.…

Q: 2. Calculate the pH at each stage in the titration for the addition of 0.110 M HCL to 35.0 mL of…

Q: Calculate the pH of a titration of 50.00 mL of 0.100 M Phenylacetic acid, Ka = 4.9 x 10-5, with…

A: The relation for ionic product of water is as follows, Kw = Ka × Kb The…

Q: Calculate pH at 0 mL NaOH added, 6.5 mL NaOH added, 14.25 mL added, and 23.50 mL added. 120 mL of…

A: we need to calculate the pH of solution

Q: Answer the following questions based on this titration curve. Assume that all laboratory work was…

A: The titration curve given is,

Q: A 24.9mL sample of 0.132 M HCI is titrated with 0.253 M NaOH. Calculate the pH after the addition of…

Q: 1. This titration curve could represent 20 ml of 0.1 M with 0.1 M NaOH. The buffer region(s) is/are…

A: We are given the titration curve for the titration of an acid with strong base, NaOH.

Q: 6. Calculate the pH of a solution during a titration of 2.5M HCI with 35mL of 1.25M NaOH A. 12mL of…

A: Given: The molarity of HCl = 2.5 M The molarity of NaOH = 1.25 M The volume of NaOH = 35 mL

Q: In the titration of a strong acid with a strong base, how do you calculate these quantities?a.…

Q: exactly 25ml of 0.01 hcl was taken diluted with sufficient quantity of water to measure 250 ml and…

A: Hello. Since your question has multiple sub-parts, we will solve the first three sub-parts for you.…

Q: 40.00 mL of 0.09M NaOH is diluted to 100 mL and titrated with 0.1M HCl. Calculate the pH after the…

Q: The next 9 questions are related to the titration of 20.00 mL of a 0.0750 M acetic acid solution…

A: The equation for neutralisation reaction between acetic acid and KOH is:

Q: pH after the following volumes of a monoprotic strong acid that is 0.035M are titrated into 25.00 ml…

A: Given,Molarity of weak base = 0.025 MVolume of base = 25.00 mLKb of base = 3.4 x 10-9Molarity of…

Q: Draw the titration curve for a strong acid (titrant) and a strong base (analyte) titration. Kindly…

Q: Determine the pH during the titration of 14.4 mL of 0.130 M perchloric acid by 7.26E-2 M sodium…

Q: A 28.3 ml sample of 0.130 M formic acid (HCHO2) is titrated with 0.130 M NAOH, Calculate the pH…

Q: 4. A 25ml of 0.01M NAOH was titrated with 0.01M HCI. Calculate the pH at: a) The start before HCl…

A: When NaOH reacted with HCl, the reaction is as follows: NaOH + HCl → NaCl + H2O Volume of NaOH =…

Q: The next 9 questions are related to the titration of 20.00 mL of a 0.0750 M acetic acid solution…

A: When an acid and a base reacts, they undergo neutralisation reaction to form salt and water. In the…

Q: A 150.0 mL sample of 0.21 M HF is titrated with 0.50 M NaOH. Determine the pH at these points: At…

Q: When 40.00 mL of 1.000 M HCl is titrated with 0.6789 M NaOH, the pH increases. a.) How many…

A: Part a: Number of moles of HCl = 1 M × 0.04 L = 0.04 mol Concentration of NaOH = 0.6789 M Let the…

Q: Calculate the pH when 3.00 M HCl is used to titrate 50.0 mL of 1.50 M NaOH a.) initial b.) before…

A: Please note: As per our company guidelines we are supposed to answer only three parts of one…

Q: Calculate the pH of a titration of 50.00 mL of 0.100 M Phenylacetic acid, Ka = 4.9 x 10-5, with…

A: Since you have posted a question with multiple sub- parts, we will solve first three sub- parts for…

Q: An industrial chemist studying bleaching and sterilizing prepares a hypochlorite buffer using 0.250…

Q: Calculate. If you have 150 ml of 1 M ammonia solution (pKa=9.25). What volume of 1 M hydrochloric…

Q: 3. What is the pH of a buffer produced by mixing 225 mL of 0.305 M HCOOH with 175 mL of 0.141 M…

A: Answer: Buffer solution is a type of solution that resists the change in its pH on adding small…

Q: Determine the resulting pH when 0.003 mol of solid NaOH is added to a 100.0 mL buffer containing…

A: Hello. Since your question has multiple sub-parts, we will solve the first three sub-parts for you.…

Q: A 40.0 mL sample of 0.300 M formic acid is titrated with 0.200 M NaOH. Calculate the pH after 70.0…

A: Given, 40.0 mL sample of 0.300 M formic acid is titrated with 0.200 M NaOH.

Q: If 30 ml of 0.15 M HOCE is titrated with 0.20 M NAOH, I) Write a balanced equation for the reaction…

Q: 36.4 mL sample of a 0.110 M solution of NaCN is titrated by 0.160 M HCl. K, for prior to the start…

A: The question is based on the concept of titrations. we are titrating a weak base with a strong…

Q: DIA For each combination of acid and base below, what is the relative pH at the equivalence point of…

A: 1) Acidic Salt- strong acid+ weak base 2)Basic Salt - strong base + weak acid 3) Neutral Salt -…

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

100%

Exercises:
1. A 40.00 mL sample of 0.250 M KOH is titrated with 0.200 MHI using phenol red as the
indicator (pH range 6.4 - 8.2). Calculate the pH for the following points in the titration.
Hint: first calculate the mol of KOH remaining
Total L of
HI added
0.00
0.0250
0.0500
0.1000
mol of HI
added
0.00
mol of OH-
remaining
mol of excess H+
[OH-]remaining, M
[H+] excess, M
pH
POH

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: General Formulas in Titrations

VIEW

Step 2: pH calculation when 0.00 L HI is added

VIEW

Step 3: pH calculation when 0.025 L HI is added

VIEW

Step 4: pH calculation when 0.0500 L HI is added

VIEW

Step 5: pH calculation when 0.100 L HI is added

VIEW

Solution

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 6 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

2)Make a rough plot of pH versus milliliters of acid added for the titration of 50.0 mL of 1.0 M NaOH with 1.0 M HCl. Indicate the pH at the following points and tell how many milliliters of acid are required to reach the equivalence point. a)Before the titration starts b)At the equivalence point c)After an additional 10.0 mL of HCL is added after the equivalence point (i.e. equivalence point volume + 10.0 mL)
ANSWER D and how would the rankings change if...
100 mL of 0.18 M NaOH is titrated with 0.18 M HCl. Calculate the pH after a) 0 mL HCl b) 15 mL HCl c) 150 mL HCl
A 28.1mL sample of 0.108 M HCI is titrated with 0.175 M NAOH. Calculate the pH after the addition of 36.8 mL of NaOH. Hint: Determine the equivalence point so you know where you are in the titration. Report your answer with two places past the decimal point. Type your answer..
Determine the pH at the point in the titration of 40.0 mL of 0.200 M HNNH2 with 0.100 M HNO: after 10.0 mL of the strong acid has been added. The value of Kb for H2NNH2 is 3.0 x 10-6. PREV 1 2 4 NEXT > Based on your ICE table and definition of Kb, set up the expression for Kb in order to determine the unknown. Do not combine or simplify terms. = 3.0 x 10-6 RESET [0] [0.200] [0.0200] [0.100] [0.140] [0.175] [x] [2x] [0.200 + x] [0.200 - x] [0.0200 + x] [0.0200 - x] [0.100 + x] [0.100 - x] [0.140 + x] [0.140 - x] [0.175 + x] [0.175 - x]
For each scenario below, select the color of the solution using the indicator thymol blue during the titration. When you first add indicator to your Na2CO3 solution, the solution is basic (pH ~10), and the color is [Select] At the equivalence point for the titration, the moles of added HCI are equal to the moles of Na2CO3. One drop (or less!) past this is called the endpoint. The added HCI begins to titrate the thymol blue indicator itself. At the endpoint, the indicator color is [Select] When you weren't paying attention and added too much HCI (~12 mL extra), the color is [Select] When you really weren't paying attention and reached the second equivalence point of Na2CO3, the color is ✓ [Select] blue yellow red orange green Question 9
Draw the titration curve, when 40.00 mL of 0.22 M ammonia solution is titrated with 0.50 M HCl. As with this does not need to be 100% perfect, but should correctly represent the important characteristics such as shape of the curve and pH values at the 4 distinct locations: Beginning, buffer region, equivalence point, beyond plateau.
1. Calculate the amount of phosphoric acid and phosphate salts (sodium phosphate, sodium hydrogen phosphate , and sodium dihydrogen phosphate). Assume you will need approximately 500mL of each buffer. The two buffers are 0.010M phosphate buffers at two pH levels of 2 and 6.
Consider the situation in which 50.0 mL of 0.200 M HNO3 is being titrated with 0.100 M NaOH. Determine each quantity: 3. determine the pH after adding 20.0 mL of base
25.0 ml of 0.100M NaOH is titrated with HC2H3O2 and 50.0mL of the acid is used to reach the endpoint. e)Would the compound formed at the equivalence point be acidic, basic or neutral? Write a hydrolysis equation for the salt formed in a) to support your answer. f) Which indicator should be used for this titration? g)Sketch a titration curve for this reaction. Label the x and y axes.
A 10.0 ml. solution of 0.300 M NH, is titrated with a 0.100 M HCl solution. Calculate the pH after the following additions of the HCI solution: 0.00 ml., 10.0 ml., 30.0 ml., and 40.0 ml.. Round your answer to 3 decimal places. Note: Reference the K, of acids at 25 °C and K, of bases at 25 °C tables for additional information. Part 1 of 4 0.00 ml. Added, pH= Part 2 of 4 10.0 mL Added, pH = 0.. 0.8
Let HA represent a weak acid. A 10.0 mL sample of 0.600M HA was titrated with 0.300 M NaOH. The table below is some of the data for this titration. Volume NaOH added (mL) 5.00 10.00 15.00 ? ? pH 6.98 7.46 7.93 ? ? Calculate the following: a) The volume of NaOH needed to reach the equivalence point is mL. (Report value to the correct number of significant figures.) b) The Ka for HA is Report value using no superscripts. For example, Kw = 1.0 x 10-14 or 1.0e-14 (Report value to the correct number of significant figures.) c) The Kp for A is Report value using no superscripts. For example, Kw = 1.0 x 10-14 or 1.0e-14 (Report value to the correct number of significant figures.) d) The pH of the solution at the equivalence point is e) On your sheet of paper, draw a reasonable diagram of the complete titration curve. Label both axis appropriately. Label the volumes and pH values at the MIDPOINT and the EQUIVALENCE POINT.