4 4. Recall that deprotonation is required to form a water-soluble salt and thus achieve an extraction. Thefraction of the acid and its conjugate base at different pH values can be calculated using the K. Thisinformation can be summarized on graph called a speciation diagram. This is a plot of the fraction ofdiflerent species (compounds or ions) vs. pH. A fraction of 0 indicates the substance is not present, anda fraction of I indicates that is the only substance present. The diagram for benzoic acid is below.Figure 1. Speciation diagram for benzoic acid0.80.60.40.212 3 46.7.8.9 10 11 12 13 14pH 3The pH of a 1 M NaHCO, solution is 10.5. What is dominant at this pH, benzoic acid (the conjugateacid) or benzoate (its conjugate base)?fraction of species

Weak acid is that which does not dissociates completely in aqueous solution, rather maintain…

Answered: The pH of a 1 M NaHCO, solution is…

The pH of a 1 M NaHCO, solution is 10.5. What is dominant at this pH, benzoic acid (the conjugate acid) or benzoate (its conjugate base)? & Hd

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: The value of Ka for benzoic acid is 6.30×10-5. What is the value of Kb, for its conjugate base,…

Q: A solution is prepared at 25 °C that is initially 0.25M in methylamine (CH,NH,), a weak base with…

Q: Succinic acid (H2C4H6O4), which we will denote H2Suc,is a biologically relevant diprotic acid with…

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

Q: A solution is prepared at 25 °C that is initially 0.45M in methylamine (CH,NH,), a weak base with…

A: Solution- Here we have basic buffer with Kb ; basic ; CH3NH2=0.45 M Acid; CH3NH3Br = 0.49M Kb= 4.4…

Q: a) Define and write the expression of Kw for the dissociation of water (H2O). Kw is the…

A: expression of Kw for the dissociation of water (H2O). ph of KOH aq kw

Q: of

A: According to the question, we need to calculate the pH of the following solution. A. Here, pOH =…

Q: Complete the following acid-base reactions: HCI + NaOH H2SO4 + H2O –→| In case you need to…

A: Acid-base titration is a type of quantitative analysis in which an unknown concentration of a base…

Q: A solution is prepared at 25 °C that is initially 0.46M in benzoic acid (HC,H,CO,), a weak acid with…

Q: The Ka for benzoic acid is 6.5 × 10¯. Calculate the pH of a 0.10 M benzoic acid solution.

A: Benzoic acid is monoprotic and a weak acid. It partially ionize in solution to produce C6H5COO- and…

Q: A 0.107 M solution of Providenol, a weak acid, has a measured pH of 4.32. Determine the pKa of…

A: The equilibrium constant depicting dissolution of either weak acids/base is known as dissociation…

Q: What is the pH of a solution that is 0.21 M CH3NH2 (methylamine) and 0.31 M CH3NH3Cl (methylammonium…

A: Since CH3NH2 is a weak base with pKb = 3.38 And the solution is having CH3NH2 and its conjugate acid…

Q: The weak acid HZ has a Ka of 2.55x10-4.(a) Calculate the pH of 0.075 M HZ.(b) Calculate the pOH of…

A: Given: Ka for HZ = 2.55 x 10-4 Since HZ is a weak acid, it will not get dissociated completely into…

Q: The pOH of an aqueous solution at 25°C was found to be 5.90. The pH of this solution is . The…

A: The pH ,hydronium ,hydroxide ion concentration is as follows.

Q: When titrating 15 mL of hydrazoic acid (HN3) 0.000489 mol/L, with KOH 0.000517 mol/L: What is the…

A: Here we are required to find the pH of the solution

Q: 0.00026 moles of acetic acid is added to 2.5L of water. What is the pH of the solution?

A: Acetic acid also called Ethanoic acid(CH3COOH )is a weak acid and on ionization it does not fully…

Q: .: calculate the percent dissociation of acetic acid in a solution 0.2 M in НС-Н,02 and 0.1 М HCI…

A: Answer:- This question is answered by using the simple concept of dissociation of weak acid in the…

Q: Quinine (C20H24N2O2) is the most important alkaloid derived from cinchona bark. It is used as an…

Q: Paracresol (CHROH) has a Ka- 5.5 x 1011. if 100.0 mL of a 0.5000 M aqueous paracresol solution is…

A: pH is used to determine the concentration of hydronium ion.

Q: Calculate the pH of a 0.15M solution of sodium acetate (CH3COONa). What is the percent hydrolysis?…

A: A strong base and weak acid react to form salt and water. The salt will be basic in nature and the…

Q: 2) The PH of asolution of aweak ronoprotic ucid (HA) is 2.85 what is the Ka of the acid ? Ans.: 2*10

A: Given , Concentration of weak mono protic acid ( C ) = 0.1 M pH of the weak acid = 2.85 Acid…

Q: Suppose that a benzoic acid (C,H,COOH) solution has a pH of 3.15. Which of these substances would…

A: Given substances: KCl C6H5COONa NaI HBr We have to find the substance that would increase the pH…

Q: A solution is prepared at 25 °C that is initially 0.29 M in trimethylamine ((CH,),N), a weak base…

Q: A 0.063 M solution of hydroxybenzene has pH 5 5.60. Find pKa for this acid.

A: pH = 5.60 Concentration of H3O+ can be calculated as follows: pH = -log…

Q: A solution is prepared at 25 °C that is initially 0.44 M in methylamine (CH, NH,), a weak base with…

A: Methylamine is weak base and Methyl ammonium bromide is its salt.so the solution is buffer solution.…

Q: What is the pH of a 0.64 M solution of phenol, a weak organic acid?

A: Given: Concentration of phenol = 0.64 M Ka of phenol = 1.3×10-10

Q: What is the pH of a solution that is 0.26 M CH3NH2 (methylamine) and 0.38 M CH3NH3Cl (methylammonium…

A: The basic buffer may be explained as the solution mixture which hold the weak base along with its…

Q: What volume (in mL) of 15.8 M HNO3 would be required to make 500.0 mL of a solution with a pH of…

A: Here, we have to find the volume of 15.8 M HMNO3 that would be required to make 500.0 mL of a…

Q: A certain weak base B has a base-ionization constant Kb of 5.9 × 10–4 at 25°C. If strong acid is…

A: Ionisation constant Kb of base B=5.9×10-4

Q: A 0.100 M weak base has a pH of 8.77. What is the Kb value of this base?

A: Given:Let the acid be : MOHpH=8.77also, concentration of weak base= 0.100Mi.e [MOH] =0.100M

Q: The pH of 0.010 M trimethylamine is 10.78 at 25 oC. What is the hydroxide ion [-OH] concentration?

A: pH is defined as the negative logarithm to the base 10 of hydrogen ion concentration. pH = -log10[…

Q: - solution is made from 0.19 M CH3NH2 (a weak base) and 0.27 M CH3NH3CI. What is the pH of the…

A: Solution- CH3NH2=0.19 MCH3NH3Cl=0.27MUsing the henderson eqution -GivenKb=4.4×10-4 pKb=-logKb…

Q: A 0.25-M weak base solution has a pH of 11.50. Calculate its Kb.

Q: A solution is prepared at 25 °C that is initially 0.39M in chloroacetic acid (HCH,CICO,), a weak…

Q: Calculate the percentage of ionize and unionized forms present in the following solution. Assume…

A: Weak acids partially dissociates so there is degree of dissociation alpha.

Q: Complete the neutralization reaction below: NaOH + HCI - Н-0 O. HCI Ob HNa Oc NaCl O d CIOH

A: Neutralization reaction can be defined as the chemical reaction between an acid and base to produces…

Q: he pOH of an aqueous solution at 25°C was found to be 8.10. The pH of this solution is _____ . The…

A: pH is given by the negative logarithm of the concentration of proton. pH = -log[H+] pOH is given by…

Q: 6. How many moles of benzoic acid (HC-HsO2) must be used to prepare 500. mL of a solution that has a…

Q: Arrange the following in in order of increasing base strength. 1 = weakest, 4 = strongest A) HPO42-…

A: We know that, conjugate base of strong acid is weak. Thus,

Q: A. One simple way to measure the [H] is to measure pH. If a 10.0mL solution of "acid rain" is…

A: In mixture of strong acid and weak acid pH depends on H+ ion concentration of strong acid.

Q: How many moles of conjugate base should be added to 315 mL of 0.45 M HLac to give a pH of 4.00?

A: pKa of HLac = 3.85 Moles of HLac = 0.45 x 0.315 = 0.14175 mol Let moles of conjugate base ( Lac- )…

Q: Q6) 200 ml , o.0ol M NAOH is udded to 30oml, o.0005 M HCL. what is the PH of the Soluution ? Ans. :…

A: The balanced Chemical Reaction between HCl and NaOH is - HCl + NaOH ----> NaCl + H2O Here, one…

Q: A solution is prepared at 25 °C that is initially 0.44M in ammonia (NH,), a weak base with K,= 1.8 x…

Q: [H+] and pH

Q: Q2// 1000 ml of o.1M hydrochloric acid were added to 1000 ml of o.1M ammonium hydroxide, ammonium…

A: When the salt of strong acid is weak base is formed, pH is calculated using the formula, pH=7-…

Q: A solution is prepared at 25 °C that is initially 0.38M in methylamine (CH;NH,), a weak base with K;…

A: We will calculate the pH of the solution .

Q: Calculate the percentage of ionize and unionized forms present in the following solution. Assume…

Q: 1. At 25°C, a 50mL solution is found to contain 20% by mass acetic acid (CH3COOH). The density of…

Q: The weak acid HZ has a Kₐ of 2.55X10⁻⁴.(a) Calculate the pH of 0.075 M HZ.(b) Calculate the pOH of…

A: For weak acid HZ , pKa = -logKa = -log (2.55 x 10⁻⁴) = 4 -log2.55 = 4 - 0.40 = 3.60 (a) pH of…

Q: How many liters of 0.54 M monoprotic weak acid HA should be added to 685000L of water (pH = 7.00) to…

A: Given data set: Molarity of monoprotic weak acid = 0.54 M Volume of water = 685000 L Required pH =…

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

4. Recall that deprotonation is required to form a water-soluble salt and thus achieve an extraction. The
fraction of the acid and its conjugate base at different pH values can be calculated using the K. This
information can be summarized on graph called a speciation diagram. This is a plot of the fraction of
diflerent species (compounds or ions) vs. pH. A fraction of 0 indicates the substance is not present, and
a fraction of I indicates that is the only substance present. The diagram for benzoic acid is below.
Figure 1. Speciation diagram for benzoic acid
0.8
0.6
0.4
0.2
12 3 4
6.
7.
8.
9 10 11 12 13 14
pH 3
The pH of a 1 M NaHCO, solution is 10.5. What is dominant at this pH, benzoic acid (the conjugate
acid) or benzoate (its conjugate base)?
fraction of species

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

Explain in details what happens in a buffer solution, taking note of the changes and the buffer capacity of acid and base solutions. How do you calculate the total ph change in an experiment that involves five trials.
Hydrogen sulfide (H2S) is an odorous gas that can be stripped from solution by bubbling air through the solution. H2S when dissolved in water is also a weak acid that can deprotonate to bisulfide ions which are not removed by air stripping. That reaction is ?2?--> H^+ + ??^- With equilibrium constant Ka=0.86x10-7.Find the fraction of hydrogen sulfide in the H2S form at pH 6 and pH 8. At which pH would you expect to have an easier time to strip away H2S gas?
What is the predominant form of ammonia in a solution at pH 7.0? Approximately what fraction is in this form?
This question concerns the changes which take place when a 0.1M solution of sodium hydroxide is added to 25cm3 of 0.1M hydrochloric acid. In 3 separate experiments, changes in temperature, pH, and electrical conductivity did take place in the cell, respectively. On the axes below, use broken lines(------) to indicate the results you would expect if 0.1M ethanoic acid were used instead of hydrochloric acid. Temperature arbitrary scale against Volume of alkali in cm3 pH against alkali in cm3 Conductivity against alkali in cm3
A mixture of NaCl, SiO2, and CaCO3 is separated following the procedure given in this experiment. Indicate how each of the following procedural changes would affect the amount of the specified substance recovered. Briefly explain. Hint: Refer to Table 1 for Solubility & Reactivity The recovery of CaCO3 was attempted by adding 3M H2SO4 instead of 3M HCl to the SiO2/CaCO3 residue.
Using --> as a reaction arrow, please write the complete reaction for the second procedure: AND the net ionic reaction as well
Phosphoric acid is triprotic with the step-wise dissociation shown below. A 0.92 M phosphoric acid solution is prepared. Calculate the equilibrium concentrations of the species indicated. Report all answers in scientific notation using 2 sig figs. Rather than use the quadratic equation, you can make assumptions like we do in class (ie if K<<1, then 0.1-x ~ 0.1) H3PO4H3PO4 + H2OH2O ↔↔ H2PO−4H2PO4- + H3O+H3O+ Ka1=7.5x10−3Ka1=7.5x10-3 H2PO−4H2PO4- + H2OH2O ↔↔ HPO2−4HPO42- + H3O+H3O+ Ka2=6.2x10−8Ka2=6.2x10-8 HPO2−4HPO42- + H2OH2O ↔↔ PO3−4PO43- + H3O+H3O+ Ka3=4.8x10−13Ka3=4.8x10-13 What is the pH of this solution? Report pH as a number and not in scientific notation.
Phenol Red: What is the purpose of this test? Why is a Durham tube inverted inside the test tube? At what pH does phenol red register an acidic result? What is the color? What is the color of an alkaline result? If you see an acid result, what does this mean? What about an alkaline result?
Rank in order of increasing bascity.
The first step in purifying the urine collected on the ISS is to treat every liter of urine with 20 mL of 1.0 M H2SO4. To simplify the calculations, lets assume that urine is water. a) What is the pH of a solution of 20. mL of 1.0 M H2SO4 added to 1.00 L water? To determine this, you can safely assume that 100% of the H2SO4 reacts to form H3O+ and HSO4- ions. Use pKa2 (1.92) to determine if any more protons are added to the solution from HSO4-.
The maximum buffering capacity is nearest to the pKa of the buffer. Explain why?
Calculate the concentration of A when chemical AB is dissolved in pure water. Ksp = 0.00001331 AB2(s) ⇌ A2+(aq) + 2B¯(aq) Enter answer to 3 sig figs using exponential format.