Use an Excel spreadsheet to generate a titration curve for 50.00 mL of 0.0200 M ammonia (K = 1.76 x 10) titratedwith 0.100 M HCI. Report the fraction of titration (4) and the volume of acid (V,) required at the following pH values of%3Dthe titration.pH = 10.01pH = 10.01%3!ml.pH = 8.10%3DpH – 8.10V. -ml.pH = 4.00%3DpH - 4.00V =ml.pH - 225pH= 2.25V.-ml.

given data are- volume of base=50ml molarity of base= 0.0200 M molarity of acid = 0.100M volume of…

Use an Excel spreadsheet to generate a titration curve for 50.00 mL of 0.0200 M ammonia (K = 1.76 x 10) titrated with 0.100 M HCI. Report the fraction of titration () and the volume of acid (V) required at the following pH values of %3D the titration.

Use an Excel spreadsheet to generate a titration curve for 50.00 mL of 0.0200 M ammonia (K = 1.76 x 10) titrated with 0.100 M HCI. Report the fraction of titration () and the volume of acid (V) required at the following pH values of %3D the titration.

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter8: Polyfunctional Acids And Bases

Section: Chapter Questions

Problem 10P

See similar textbooks

Related questions

Q: Sketch a titration curve and give the suitable indicator for the following condition of titrotion:…

A: Please find your solution below : It is known that acetic acid is a weak acid and sodium hydroxide…

Q: A titration curve of 30.00mL of a weak acid HX with 0.150M NAOH is illustrated below. Based on it,…

A: 30.00 mL of a weak acid HX is titrated with 0.150 M NaOH . Here we have to calculate- a. the HX in…

Q: How would prepare 750ml of 0.1M NaCl, 0.5M Tris-HCl solution given that you have 5M NaCl and 1M…

A: Molarity is defined as the moles of solute present per liter of solution. For example: 5 M NaCl…

Q: 5. A 100.0 mL aliquot of 0.100 M diprotic acid H2A (pK1 = 4.00, pK2 = 8.00) was titrated with 1.00 M…

A: Solution- Given-pK1 = 4.00 and pK2 = 8.00, 0.100 M diprotic acid, 1.00 M NaOH aliquot = 100.0ml

Q: construct a curve for the titration of 25.00-mL 0.1000 M sodium carbonate with 0.1000 M HCl

Q: A 30.0 mL sample of 0.165 M propanoic acid (Ka = 1.3x10^-5) is titrated with 0.300 M KOH. Calculate…

Q: A weak base, ammonia, is to be titrated with hydrochloric acid. A volume of 30.0 mL of the 0.75 M…

A: Answer: This is the question based on acid-base titration where weak base is the analyte and strong…

Q: A titration is carried out for 25.0 ml of 0.300M HA (Ka - 3.5 x 10) with 0.300M NAOH. Calculate the…

Q: A student titrates a 50.00mL sample of water with 17.85mL of 0.0100M ethylenediaminetetraacetic acid…

A: Given: Volume of water sample = 50.00 mL Voluime of ethylenediaminetetraacetic acid (EDTA) =…

Q: Generate a titration curve for 25 mL of 0.1200 M formic acid titrated with 0.0800 M KOH

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

Q: A chemist titrates 120.0 mL of a 0.5503 M acetic acid (HCH,CO,) solution with 0.1001 M NAOH solution…

A: Answer: In this question we have to calculate the pH of salt solution where salt is made of weak…

Q: Find the molarity of a sulfuric acid solution when 25.00 mL of this solution is titrated to a slight…

A: We will calculate molarity of sulfuric acid

Q: In the titration of 50 mL of 0.1 M HCI with 0.1 M NaOH using methyl orange as an indicator, the end…

A: Answer: Indicator is a chemical substance that indicates the completion of titration by changing its…

Q: What is the region of titration reached upon adding 10mL of 0.25M AgNO3 to 50mL of 0.15M chloride…

A: Regions of titration can we determined by four ways first is when titrant is not added to the…

Q: Solve for the pH level of an ammonia buffer. Given that it contains 500.0 mL of 0.3701 M ammonia and…

Q: Calculate the volume of 0.120M hydrocyanic acid, HCN (K, -4.9 x 10-10) solution, needed to prepare…

Q: An indicator (Ka = 1.0 x10°) where HInd is yellow and Ind is blue is added to 100.0 mL of 0.10 M…

A: Given: Indicator (Ka=1.0 x 10-9) Volume of 0.1 M HCL = 100 ml, Hind is yellow and Ind- is blue We…

Q: Calculate the pH value when titrated between 25 ml of weak acid HA with concentration of 0.3 (104 x…

Q: Consider the titration of 60.0 mL of 0.200 M pyridine with 0.400 M HCl. What is the pH at 0.00 mL,…

A: Value of pH is used to measure the acidity or basicity of a solution. At room temperature, value of…

Q: Determine the pH during the titration of 39.6 mL of 0.226 M trimethylamine ((CH3)3N, Kp = 6.3x10-5)…

A: Since you have asked a question with multiples of parts we will answer only 1st 3 subparts for you.…

Q: Calculate the equivalence point volumes for a titration of 25.00 mL of 0.060 M HCl and 01.0 M H3PO4…

A: HCl vs NaOH Volume of HCl ( Va ) =25.00 mL Molarity of HCl ( Ma ) = 0.060 M Molarity of NaOH ( Mb…

Q: Construct the titration curve for the titration of 26.0 mL of 0.100 M KOH with 0.0600 M HNO3

Q: Consider the titration of 50.0 ml. of 0.350 M NH3 (K, 1.74x10 5) with 100 mM HCI. What will the pH…

A: Since you have posted multiple questions, as per our company guidelines we are supposed to answer…

Q: The Ka of Benzoic acid (C6H5COOH) is 6.3 x 10-5. A 0.72 M C6H5COOH of 40.0 mL is titrated with 0.48…

A: Option C The answer for (1) 30.0 ml and the answer for (2) 60.0 ml

Q: Consider the titration of 20.0 mL of 0.100 M perchloric acid with 0.400 M LiOH. What is the pH and…

Q: 50mL of 0.025 M HF is titrated with 0.045 M NaOH. a) What amount of NaOH is required for…

A: amount of NaOH is required for equivalency point = 27.77 mL

Q: Consider the titration of 30.0 mL of 0.050 M NH3 with 0.025 M HC1. Calculate the pH after the…

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

Q: IKalculute the pH and plot the resulting titration curve for Hhe titration of 20ml, o.1l M ammonia…

Q: if 150. ml of 0.50 M formic acid (HCOOH) is titrated with the strong base of 0.50 M. KOH (Ka for…

A: Given: The volume of 0.50 M formic acid used for titration is 150.0 mL. The volume of 0.50 M KOH…

Q: Construct a rough plot of pH versus volume of added base for the titration of 50 mL of 0.045 M HCN…

Q: 4. A solution of hydrofluoric acid (0.27 M, 10.00 mL) was titrated with 15.0 mL of 0.13 M sodium…

A: Given: Molarity of hydrofluoric acid is 0.27 M. Volume of hydrofluoric acid is 10.00 mL. Molarity of…

Q: Calculate and sketch qualitatively correct titration curves for the following acid – base reaction:…

A: Given : Volume of KOH = 25.0 ml Molarity of KOH = 0.100 M Molarity of HNO3 = 0.05 M

Q: Sketch the titration curve that will be obtained when 50 mL of 0.05 M glycine at pH 1.5 is titrated…

A: Equivalence point: It is a point in titration at which the amount of titrant added is just enough to…

Q: A 25.0 mL sample of 0.100 M acetic acid is titrated with0.125 M NaOH at 25°C. What is the pH of the…

A: Moles are calculated.

Q: 30 cm3 of 0.5 M solution of weak monoprotic acid titrated with 10 cm3 of a 1 M NaOH solution. If the…

Q: 500 ml of 0.1019 M NaOH solution is prepared It is immediately forgotten with the cap open and…

A: NaOH reacts with carbon dioxide as: 2NaOH+CO2→Na2CO3+H2O

Q: In the titration curve below, which species would NOT be in solution at Point B? Unknown Solution…

A: In the given graph, at B point pH=11

Q: A 250.0-mg sample of an organic monoprotic weak acid was dissolved in an appropriate solvent and…

A: Ratio of number of gram equivalents present in the solution to the volume of the solution in liter…

Q: Consider the titration of 40.0 mL of 0.20 M H3A (K = 3.0 x 10-4,. , K. 4.4 x 10-8, K = 8.0 x 10-11)…

A: Calculation of no. of mol of H3A: n=Molarity×Volume=0.20 mol/L×40.0×10-3 L=8×10-3 mol Calculation of…

Q: What do you call the stage of the titration in which the number of moles of the titrant is…

A: We have to tell the name of the stage when the number of moles of the titrant is stoichiometrically…

Q: Consider the titration of 50.0 mL of 0.350 M NH3 (K, = 1.74x10 5) with 100 mM HCI. What will the pH…

A: The balanced equation is NH3 + HCl ----------> NH4+Cl– Given that concentration of HCl =100 mM…

Q: When titrating a weak acid with a strong base, what is the approx. pH expected for the equivalence…

A: The pH of a solution is the negative logarithmic of H+ ion concentration in the solution.

Q: Consider the titration of 12.0 mL of 0.24 M hydrochloric acid (as the analyte) and 0.40 M sodium…

A: Given: Volume of HCl = 12.0 mL Molarity of HCl = 0.24 M Volume of NaOH = 10.0 mL Molarity of NaOH =…

Q: An indicator (Ka = 1.0 x10°) where HInd is yellow and Ind is blue is added to 100.0 mL of 0.10 M…

Q: Consider the titration of 20.0 mL of 0.100 M perchloric acid with 0.400 M LiOH. What is the pH and…

Q: Calculate the relative carbonate error made in acetic acid titration

A: According to question Concentration of NaOH = 0.1019M Volume of NaOH = 0.5L No. Of moles of NaOH…

Q: 4. A 100.0-mL solution consisting of 0.14 M NaC2H30z and 0.16 M HC2H302 was titrated with 24 mL of…

A: 4. Millimoles of KOH = M x V = 0.25 x 24 = 6 mmol Millimoles of HC2H3O2 = M x V = 0.16 x 100 = 16…

Q: 25.0 ml of 0.100M NaOH is titrated with HC2H3O2 and 50.0mL of the acid is used to reach the…

A: An acid base titration gives salt and water as product. This reaction is called a neutralization…

Q: Consider the titration of 50.0 ml of 0.350 M NH3 (K, 1.74x10 5) with 100 mM HCI. What will the pH be…

A: Since you have posted multiple questions, as per our company guidelines we are supposed to answer…

Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

Use an Excel spreadsheet to generate a titration curve for 50.00 mL of 0.0200 M ammonia (K = 1.76 x 10) titrated
with 0.100 M HCI. Report the fraction of titration (4) and the volume of acid (V,) required at the following pH values of
%3D
the titration.
pH = 10.01
pH = 10.01
%3!
ml.
pH = 8.10
%3D
pH – 8.10
V. -
ml.
pH = 4.00
%3D
pH - 4.00
V =
ml.
pH - 225
pH
= 2.25
V.-
ml.

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

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 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

Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a) before any NaOH is added? (b) at half-neutralization? (c) at the equivalence point? (d) when 0.10 mL less than the volume of NaOH to reach the equivalence point is added? (e) when 0.10 mL more than the volume of NaOH to reach the equivalence point is added? (f) Use your data to construct a plot similar to that shown in Figure 14.10 (pH versus volume NaOH added).
The next 11 questions are related to the titration of 30.00 mL of a 0.1000 M acetic acid solution with 0.0800 M KOH. Assume that the temperature is 25 oC.What is the initial pH of the analyte solution? What volume of KOH is required to reach the equivalence point of the titration? How many mmol of acetate are present at the equivalence point? Report the analytical amount, not the equilibrium amount of acetate at the equivalence point. What is the total volume of the solution at the equivalence point?
Mercury thiocyanate - Hg(SCN)2 - is slightly soluble in water. Its Ksp is 2.8 x 10-20. In the titration of 50.00 mL of 0.0457 M Hg2+ with 0.200 M SCN-, show or calculate the following: ii. The volume of SCN- needed to reach the equivalence point (Ve).
A 250.0-mg sample of an organic monoprotic weak acid was dissolved in an appropriate solvent and titrated with 0.091 M NaOH, requiring 29.5 mL to reach the end point. Determine the compound’s equivalent weight.
Generate a titration curve for 25.0 mL of 0.7233 M H3PO4, with 1.256 M NaOH as the titrant, given the following total volumes of titrant dispensed. H3PO4 ⇌ H2PO4- Ka1 = 7.11 x 10 -3 H2PO4- ⇌ HPO4 -2 Ka2 = 6.32 x 10 -8 HPO4 -2 ⇌ PO4 -3 Ka3 = 4.50 x 10 -13 V NaOH (mL): 0.00, 2.0, 12.0, 20.0, 30.0, 38.0, 45.0, 57.0, 66.0, 70.0, 85.0
Consider the titration of 25 mL of 0.1 M HCHO2 (known as formic acid and has a Ka of 1.8 x 10-4) with 0.1 M of the strong base KOH. Clearly calculate the initial pH, the pH at half way to the equivalence point, the pH at the equivalence point, and the pH after the addition of infinite excess KOH.
Calculate the equivalence point volumes for a titration of 25.00 mL of 0.060 M HCl and 01.0 M H3PO4 with 0.075M NaOH. There will be two of them.
If 0.3074 g of a mixture of pure KCl and KBr requires 30.98 mL of 0.1007 M AgNO3 solution for its titration, calculate the% KCl and KBr in the sample. (Pat Data: Cl, 35.453; Br, 79.904; K, 39.098)
1) A 65 mL sample of 0.460 M acetic acid (CH3CO2H) is titrated with 0.325 M NaOH. Calculate the pH of the solution at the equivalence point. Ka for CH3CO2H is 1.8 x 10-5.
What change in pH will occur when 0.050 mmol of HOAc (Ka= 1.78 x 10^-5) is added to 100.0 ml of a buffer solution that is 0.1000 M HOAc and 0.1000 M NaOAc? Assume no change in volume.
1 ) The density of a 5.26MNaHCO 3 (84.0 g/mol) is 1.19g / m * l . Its molality is 2) Calculate the pAg^ + at the equivalence point in the titration of 25.0ml of 0.0823 M Kl with 0.051M AgNO 3 . Ksp Agl=8.3*10^ -16 3) Commercial concentrated aqueous nitric acid is 70.4% HNO3(63.0 g/mol) by mass and has a density of 1.41g / m * l . The molarity of this solution is 4) Consider the titration of 25ml of 0.0823M KI with 0.051M AGNO3, Kspagi =8.3x10-16 Calculate pAg* after adding 39.0 ml I03 Ag* + 103 ====AglO3 5) Commercial concentrated aqueous nitric acid is 70.4 1\%HNO 3 (63.0 g/mol) by mass and has a density of 1.41g / m * l . The molarity of this solution is: 6) What mass in g of Na 2 CO 3 [106 g/mol] is required to prepare 250 ml of 0.3M aqueous solution in Na^ + [23.g/mol] ? 7) Calculate pAg^ + after adding 42.30ml AgNO 3 In the titration of of 0.0823M Kl with 0.051M AgNO 3 . KspAgl = 8.3 * 10 ^ - 16 8) The milliliters of concentrated HClO 4 (100.5 g/mol),6 60% by mass,…
A solution containing 100.00 mL of 0.1800 M acetic acid (Ka = 1.78 x 10-5) is being titrated with 0.3500 M NaOH. Calculate the pH and construct a titration curve. After the addition of 25.00 mL NaOH At half-equivalence