NaCH3COO ,sodium acetate NaC6H5COO , sodium benzoate NaCH3CH2 COO sodium propionate NaHCO 3 , sodium bicarbonate 1. If methyl orange-xylene cyanole is used as the acid-base indicator in this reaction, what color change do you expect to see?

NaCH3COO ,sodium acetate NaC6H5COO , sodium benzoate NaCH3CH2 COO sodium propionate NaHCO 3 , sodium bicarbonate 1. If methyl orange-xylene cyanole is used as the acid-base indicator in this reaction, what color change do you expect to see?

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter16: Principles Of Chemical Reactivity: The Chemistry Of Acids And Bases

Section16.7: Calculations With Equilibrium Constants

Problem 16.8CYU: Calculate the pH after mixing 15 mL of 0.12 M acetic acid with 15 ml of 0.12 M NaOH. What are the...

See similar textbooks

Related questions

Q: 14. Which indicator in yellow in a solution with a pH of 987 A methyl ornge R. hromthymol Mue C…

A: We have to tell which option is correct

Q: Dilute phosphoric acid(K1 = 7.5 x 10-3) solution is titrated with standard NaOH solution to form…

A: Which indicators is used not used for this titration are given below.

Q: Which acid would you choose to combine with its sodium salt to make a solution buffered at pH 4.25?…

Q: How would you prepare a buffer solution ?give the constituent ratio of ph 8 buffering ?

A: Buffer solutions The solution that resists any change in pH is known as buffer solution. There are…

Q: How does the Eriochrome Black T indicator function?

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

Q: Calculate the pH after 0.030 mole of NaOH is added to 1.00 L of each of the following solutions. a.…

A: pH of given solutions are as follows:

Q: Assume that you have two unlabeled bottles, one of which contains phenol (pKa = 9.9) and one of…

A: Acid is a substance which is capable of donating a proton or capable of accepting lone pair of…

Q: Complete the balanced dissociation equation for the compound below in aqueous solution. AgI ->

A: The compound given is AgI.

Q: What are the concentrations of each of the following species in 1.50 M sodium oxalate, Na2C2O2?…

A: Given: Concentration of sodium oxalate, Na2C2O4 = 1.5 M Ka1 for oxalic acid = 5.9 x 10-2 Ka2 for…

Q: When ammonium sulfate dissolves, both the anion and cation have acid-base reaction: (NH4)2SO4(s)→…

A: Questions are 1. Charge balance 2. Mass balance 3. NH3 concentration calculation

Q: Fill out the chart that will illustrate the ranges of color change for the following acid-base…

A: pH is defined as negative logarithm of hydrogen ions.

Q: a volume of bore water with a pH of 8.06 was blended with an equal volume of another water sample…

A: pH = 8.06 for sample -1 pH = 6.00 for sample -2

Q: Place the missing compounds in the flow diagram for the separation of a strong acid ,a weak acid , a…

Q: 7) Oxalic acid is the simplest diprotic organic acid. How many milliliters of 0.800 M KOH should be…

A: Calculation as shown below

Q: What is the ratio of acetate ion to acetic acid (Ka = 1.76×10–5) in a solution containing these…

Q: Phosphoric acid is a triprotic acid with the p?apKa values p?a1=2.148pKa1=2.148, p?a2=7.198…

Q: 2. The colorless solution of an unknown solid turned red litmus blue. No odor was noted upon adding…

A: Given in the question that given salt sample solid turns red litmus paper into blue , thus it…

Q: Suppose you made a mistake in analysis of Ag+, Pb++ ,Hg2++ and instead of 6M HCl you added 6M HI .…

A: Given : Suppose you made a mistake in analysis of Ag+, Pb++ ,Hg2++ and instead of 6M HCl you…

Q: 3) into a 1.000 liter volumetric flask, and suddenly realize that you don’t have all the reagents…

Q: A 50.0 ml of acidic solute (K. = 1.20 x 10-2) is titrated with a 2.50 mL of x 10-5 M NaOH solution.…

A: Given: Ka of acid solute = 1.20 X 10-2 Volume of acid solution = 50.0 mL = 0.050 L…

Q: Which of the following mixtures are capable of tolerating addition of a strong base without altering…

Q: CH3COO + H2O → CH3COOH + OH- K₂=1.8x10-5(for acetic acid)

A: Given: Concentration of CH3COONa is 0.100 M Given reaction is: CH3COO-+H2O→CH3COOH+OH- Ka is…

Q: What is the ratio of acetate ion to acetic acid (Ka = 1.76×10–5) in a solution containing these…

Q: Using the reaction below, predict the effects on sulfuric acid concentration (increase/decrease) if…

A: According to Le-Chatelier's principle, if the reaction at equilibrium is disturbed, then the…

Q: bromothymol blue indicator has only one color change, from yellow (ph below 7) to blue (ph near 7).…

A: The acids which can easily donate proton are known as strong acids. More the strength of an…

Q: Use of concentrated NAOH (lye or caustic soda) in soap preparation can produce a very basic product.…

A: Saponification : It is the process where salt of fatty acid is treated with base (generally NaOH )…

Q: What is the approximate pH of a solution prepared by mixing equal volumes of 0.05 M methylamine and…

A: Given - Molarity of methyl amine = 0.05M Molarity of hydrochloric acid = 0.2M n- Volume of Methyl…

Q: what is the pH of a solution prepared by mixing 50.0 mL of 0.125 M amonia and 25.0 mL of 0.100 M…

Q: How to prepare 50 ml. 1x PBS solution (pH 7.4).

A: Phosphate Buffered Saline (PBS) : Phosphate Buffered Saline is an isotonic buffer, which is…

Q: What are some possible sources of error in determining the Ka value of an unknown acid except for…

Q: If the conjugate base or salt is not readily available, the salt is produced by reacting NaOH and…

A: Given -> Concentration of salt component = 0.5 M

Q: Phenolphthalein indicator is a weak acid with Ka = 10-9 mol/dm-3. It is colourless while its…

A: Phenolphthalein indicator is a weaker acid it's work in higher pH range between 10 to 12. In acidic…

Q: I

A: We use the indicator to judge how strong a given acid or base is used. So, lower value of pH gives…

Q: Selenic acid, H2SeO4, is a diprotic acid that actually is a strong acid for the donation of its…

A: The dissociation of weak acid is very low as compared to strong acid and base. The weak acid and…

Q: What conjugate base could be used to make a phosphoric acid (H3PO4) buffer at pH = 2? a. H2PO4^- b.…

Q: Formic acid (HCOOH) has a Ka = 1.8 × 10-4. What is the pH of a 25.00mL sample of 0.205 M formic acid…

Q: Using the chart, which of the following would be an appropriate indicator for the titration of a…

A: Indicator is used in a titration to show the equivalence point attainment by changing colour of…

Q: Draw/illustrate the chemical reaction involved in Barfoed’s test and explain the purpose of this…

Q: Phenol red is a common acid-base indicator. It has a pKa equal to 8.000. It's undissociated form is…

Q: Consider applying the systematic treatment of equilibrium to a system containing a diprotic acid.…

A: The dissociation of weak diprotic acid is expressed as, H2A⇆Ka1HA-+H+HA-⇆Ka2A2-+H+ Ka1 and Ka2 are…

Q: Titration of another 30.0 mL sample of aqueous HX with 0.111M NaOH yields the titration curve below.…

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

Q: Show a reaction equation depicting the addition of a strong acid to a buffer solution containing…

A: The buffer contain acetic acid in equilibrium with its conjugate base. Write the reaction for…

Q: What is the pH of a solution prepared by mixing 20.0 mL of 0.50 M NaOH and 35.0 mL of 0.50 benzoic…

A: A numerical problem based on pH calculation, which is to be accomplished.

Q: Methyl red (Ka = 6.3 x 10-6) is a common acid-base indicator. Its un-ionized form is red and its…

A: PKa =- log Ka Where Ka = dissociation constant

Q: Hi can you answer the following question: Using the data from questions 3 and 4, calculate the…

A: The number of moles of unknown acid is calculated as, nHA=0.042 mol/L×0.25 L=0.0105 mol The number…

Q: 7) Your lab instructor asks you to prepare 1.0 L of 0.10M buffer at pH = 5.00 exactly. If only the…

A: Given - Expected pH of buffer = 5.00 Buffer solution - 1.0 L of 0.10 M Ka values Choloracetic acid…

Q: From the Pourbaix diagram of Cu shoOwn below 1.6- 1.2+ 2 Cư 0.8 + Cu(OH),(s) 0.4- 3 Cu,0(s) Cuof…

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

Q: The Acids used in this experiment are all monoprotic. What does that tell you about the acid?…

Q: uestion 8 Based on the results obtained in the following table, which indicator has approximately a…

A: The correct option is:

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

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

VIEW

Step 2

VIEW

Step by step

Solved in 2 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

How would you prepare a buffer solution ?give the constituent ratio of ph 8 buffering ?
bromothymol blue indicator has only one color change, from yellow (ph below 7) to blue (ph near 7). why would this indicator be a poor choice to distinguish between strong and weak acids?
If the actual mass of a base used (sodium citrate dihydrate) in a buffer solution is 1.5 g, and the concentration of the acid used (5 mL, ammonium citrate) is 2 M, with a Ka of 4.06E-7, what is the concentration of this base (in M) in this buffer solution?
Calculate the pH after mixing 15 mL of 0.12 M acetic acid with 15 ml of 0.12 M NaOH. What are the major species in solution at equilibrium (besides water), and what are their concentrations?
Assume that you have two unlabeled bottles, one of which contains phenol (pKa = 9.9) and one of which contains acetic acid (pKa = 4.76). In light of your answers to Problem 8 which is the pH of a 0.050 M formic acid is 1.30, suggest a simple way to determine what is in each bottle.
Which of the following sequences show an increasing strength of acidity? I. HNO2 (Ka=4.0 x 10-4) II. HOC6H5 (Ka=1.6 x 10-10) III. HSO4- (Ka=1.2 x 10-2) IV. HCN (Ka= 6.2 x 10-10) III, I, IV, II II, IV, I, III III, I, II, IV IV, II, I, III
A student prepared a 0.10 M solution of formic acid, HCHO, and allowed it to be dissociated. The [H3O]+ was found to be 4.2 x 10-3M. What is the acid dissociation constant, Ka for HCHO?
1- How does the Eriochrome Black T indicator function? 2- What is the molecular structure of Eriochrome Black T indicator? What are the donoratoms?
phenolphthalein is an indicator that when added to a soltuion, appears clean at a ph belowe 8 and pink at a ph above 8. what color will each of the following solution appear with two drops of phenolphthalein added 1. [h3o+]-5.25*10^-4 m 2. [oh-]=6.94*10^-5 m
what is the pH of a solution prepared by mixing 50.0 mL of 0.125 M amonia and 25.0 mL of 0.100 M hyrogen chloride (The acid dissociation constant of amonnium ion is 5.70x10-10)
The Acids used in this experiment are all monoprotic. What does that tell you about the acid? Select one: a. That they have one ionizable H and react in a 1:1 ratio with OH- b. That they have a pH of 1 c. That they will react the same way a strong acid reacts with OH- and will be neutral. d. That they are a stronger acid than di or triprotic acids
What would the [OH-] be after addition of 9.75 mL of 0.1000 M HCl to 25.00 mL of 0.1000 B (a weak base, Kb = 6.05e-6)? 3.87e-6 9.46e-6 5.02 1.70e-6