Please complete the calculation of the pH of the equivalence point below. Concentration of NaOH solution = 0.1 mol dm-3. Mean titre (NaOH solution) = 18.95 cm3. Amount of NaOH = 0.00189 moles. Molar ratio of NAOH:aspirin = 1:1. Amount of aspirin = 0.00189 moles. Mass of aspirin (in titration) = 0.341 g. Mass of aspirin (per tablet) = 0.341 g. %D

Please complete the calculation of the pH of the equivalence point below. Concentration of NaOH solution = 0.1 mol dm-3. Mean titre (NaOH solution) = 18.95 cm3. Amount of NaOH = 0.00189 moles. Molar ratio of NAOH:aspirin = 1:1. Amount of aspirin = 0.00189 moles. Mass of aspirin (in titration) = 0.341 g. Mass of aspirin (per tablet) = 0.341 g. %D

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: What must be the minimum concentration of hypoiodous acid in 1.00L buffer solution of a pH=10.72…

Q: ralence point. Gi nt (in grams) of t 5738

Q: The solubility of Ni(OH)2 in a pH =7.64 solution is_, Ksp Ni(OH)2 =1.6 x 10-16. %3D

Q: A solution is prepared at 25 °C that is initially 0.48M in diethylamine ((C,H) NH, a weak base with…

Q: If NH4OH (aqueous ammonia, Kp = 1.8 x 10-5) is titrated with HCI, the pH at the equivalence %3D…

Q: The buffer in this experiment is made of acetic acid HC2H3O2 and sodium acetate NaC2H3O2 (C;H3O2 ).…

A: When NaOH solution is added to buffer solution , it would react with Acidic part of buffer solution…

Q: Which of the following mixture will not constitute a buffer solution ? a)0.1 mole HCl and 0.1 mole…

A: Buffer is a mixture of weak acid and salt formed from its conjugate base or weak base and salt…

Q: In the titration curve below, what is the pH of the solution equal to at Point D? 14 Unknown…

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: A mixture of HCl and H3PO4 is titrated with 0.100 M NaOH. The first end point (methyl red) occurs at…

A: The objective of the question is to calculate the millimoles and present in the solution.

Q: Based on the result of the acid-base reaction, set up the ICE table in order to determine the…

Q: Consider the titration of 60.0 mL of 0.0400 M NH3 (a weak base; Kb = 1.80e-05) with 0.100 M HCl.…

A: In multipart questions, we solve only first three subparts according to bartleby guidelines. To find…

Q: calculate the pH of the equivalence point N2OH soluhon Concentrahun.of n =0.lmol/L Mean titre (MOOH…

A: A titration is an analytical method that is used to determine the unknown quantity of the analyte…

Q: Sketch a titration curve and give the suitable indicato for the following condition of titration: a)…

A: (a) Solution -

Q: Determine the pH during the titration of 26.7 mL of 0.305 M benzoic acid ( Ka = 6.3\times 10 - 5) by…

A: The objective of this question is to calculate the pH at different points during the titration of…

Q: Suppose we have a formula for the titration function P(x). What calculation would we want to do to…

A: Weak acids dissociate partially in an aqueous solution to furnish the hydrogen ions. The extent to…

Q: Calculate the A 36.4 mL sample of a 0.240 M solution of NaCN is titrated by 0.290 M HCI. K, for CN…

A: The solution is shown in the image below-

Q: Calculate pH of a weak acid/conjugate base buffer solution. Calculate the pH of 540. mL of a 0.173-M…

A: Given data 540. ml of a 0.173-M HCN before and after the addition of 5.94x10-2 mol of KCN

Q: 25.0 mL of 0.25 M HCN (for HCN; Ka = 6.2 x 10-10) sample is titrated with 0.50 M NaOH. Calculate the…

A: The question is based on the concept of the pH of the solution.It is defined as a negative logarithm…

Q: Noting that the ratio of weak conjugate base(the anion of the acid) to weak acid in a titration can…

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

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

A: In acid-base titration, two terms are very common - Titrant and Analyte Titrant : A solution,…

Q: Compare conductivity titration to the pH-metric titration that you performed earlier. Do both…

A: Solution - conductivity titration - Conductometric titration is a type of titration in which the…

Q: Be sure to answer all parts. Find the pH of the two equivalence points and the volume (mL) of 0.0418…

A: Titration of 17.3 mL of 0.130 M H2CO3 with 0.0418 M KOH.We have to find out the pH of the two…

Q: The solubility of CACO, in water at 25 °C is measured to be 0.0067 . Use this information to…

A: The concentration of the calcium chloride in the solution is = 0.0067 g/L The value of the…

Q: 0.265 g Na2CO3 is weighed and 250 ml solution is prepared and 50 ml sample taken from here is…

A: Mass of Na2CO3 = 0.265 gVolume of HCl = 10.2 mLNormality of HCl = 0.1 NTo find the factor of the HCl…

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…

Concept explainers

Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

Question

Please complete the calculation of the pH of the equivalence point below.
Concentration of NaOH solution = 0.1 mol dm-3.
Mean titre (NaOH solution) = 18.95 cm3.
Amount of NaOH = 0.00189 moles.
Molar ratio of NaOH:aspirin = 1:1.
Amount of aspirin = 0.00189 moles.
Mass of aspirin (in titration) = 0.341 g.
|Mass of aspirin (per tablet) = 0.341 g.

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

Please don't provide handwritten solution... A 1.0 L solution contains 0.100 mol HC2H3O2 and 0.100 mol NaC2H3O2. The value for Ka HC2H3O2 is 1.8 X 10-5. What is the pH of the buffer after adding 0.010 mol NaOH to the buffer.
Ex. 13-5. A 50.00-mL of an HCl solution required 29.71 mL of 0.01963 M Ba(OH)2 to reach an end point with bromocresol green indicator. Calculate the molarity of the HCl. Ва(ОН)2 + 2HCІ- ВаCl, + 2H-0
A sample of NOCl decomposes according to the following equation: 2 NOCl(g) 2 NO(g) + 1 Cl2(g) An equilibrium mixture in a 5-L vessel at 209 oC, contains 0.0220 g of NOCl, 0.0114 g of NO, and 0.0533 g of Cl2.(a) Calculate KP for this reaction at this temperature.KP = _______ .
ANSWER D and how would the rankings change if...
On the following titration curve, indicate what the pH is at each point (eg. >7, =7, <7), what the major chemical species present are, and what type of solution is present Titration curve is shown on the image provided
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]
How many milliliters of 1.27 M NaOH must be added to 275 mL of 0.11 M H₂PO4 to make a buffer solution with a pH of 6.407 Round your answer to 2 significant digits. Note: Reference the pK, of weak acids at 25 °C table for additional information,
What is the highest pH that could be used as an effective buffer with B (a generic base) with Kp = (6.46x10^-10) and its chloride salt, HBCI? Enter your answer in scientific notation with 3 sig figs. Do not include any units in your answer. Do not round any intermediate calculations. Note: Your answer is assumed to be reduced to the highest power possible.
A 50.00 mL of 0.0275 M HCl solution was titrated with 0.1500 M NaOH. Calculate the pH of the analyte solution in the specified volumes of the titrant added. At 5 mL of the titrant. -1.26 -1.56 -1.86 -2.06 At 14 mL of the titrant. -10.23 -11.78 -12.23 -13.78 At 20 mL of the titrant. -10.23 -11.78 -12.23 -13.78
What is the resulting molarity of LIOH after dilution (but BEFORE any possible chemical reaction) if (2.28x10^1) mL of (9.020x10^-1) M LİOH are mixed with (5.740x10^1) mL of (3.040x10^-1) M HCI? Enter your answer in scientific notation with 3 sig figs. Do not include any units in your answer. Do not round any intermediate calculations. Note: Your answer is assumed to be reduced to the highest power possible.