Given the reaction: HPO4 2- (aq) + HC2H3O2 (aq) ↔ H2PO4 - (aq) + C2H3O2 - (aq) 1. The acid in the forward reaction is _____________. 2. The acid in the reverse reaction is_____________. 3. The base in the forward reaction is______________. 4. The base in the reverse reaction is ____________.

Given the reaction: HPO4 2- (aq) + HC2H3O2 (aq) ↔ H2PO4 - (aq) + C2H3O2 - (aq) 1. The acid in the forward reaction is _______. 2. The acid in the reverse reaction is_. 3. The base in the forward reaction is. 4. The base in the reverse reaction is ____.

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter7: Neutralization Titrations And Graphical Representations

Section: Chapter Questions

Problem 15P

See similar textbooks

Related questions

Q: what are the molar H3O+ and OH- concentrations in (a very brief but concise solution will do)…

A: 0.0300 M HOCl 0.0600 M butanoic acid 0.200 M NaOCI

Q: What is the concentration ratio of H2PO4- to HPO42- at pH = 7.05? H2PO4-(aq) ↔ HPO42-(aq) + H+(aq)…

A: According to Handarson's Equation :PH = PKa+ log HPO42-H2PO4-Given PH = 7.05Ka = 6.2 x 10-8Pka =…

Q: n the following reaction of tetrafluoroboric acid, HBF4, with acetate ion, C2H3O2-, the formation of…

A: According to Bronsted Lowry concept of acid and bases,acids are proton donors and bases are proton…

Q: Classify the following molecules (based on molecular behavior) whether they are: A. Arrhenius acid…

Q: The following scenes represent three weak acids HA(where AX, Y, or Z) dissolved in water (H₂O is…

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

Q: calculate the pH at 25°C of a 0.24M solution of sodium benzoate NaC6H5CO2. Note that benzoic acid…

A: An acidic substance is the substance that can give H+ ions. They are corrosive and sour in nature.…

Q: When ammonium (NH4+) is placed in water, a chemical reaction occurs and an equilibrium is…

A: By applying the Henderson Hasselbalch equation, we can predict the predominant form.

Q: The weak acid HQ has a pKₐ of 4.89.(a) Calculate the [H3O⁺] of 3.5X10⁻² M HQ.(b) Calculate the…

A: Calculation of dissociation constant:

Q: A 300 mL of 0.05M ammonia. The density of the solution is 0.88 g/mL. Pka pf ammonium = 9.255. What…

Q: Are there any ions that will hydrolyze in ammonium carbonate? I wrote its reaction with water and…

A: According to the Bronsted Lowry concept of acid and a base, a conjugate acid is defined as that…

Q: For acetic acid, at equilibrium: Ka- [H3O*][CH;CO2 V [CH, CO2 H] =1.8×10"s In this case, you know Ka…

A: The pH is a negative logarithm of the concentration of hydrogen ions. pH = -log H+

Q: A diprotic base (B) has pK, values of 3.33 (pK5i) and 6.66 (pK2). Which of the equalities is true…

A: Here we have to determine the predominant species of a diprotic base B at different pH. Given pKb1=…

Q: Consider the following reaction. According to Bronsted-Lowry, HCO3- is a(n): HCO3- + H2O ----> H3O+…

Q: Acid Conjugate base Acid H2SO3 HSO3 Base Strength Increases Strength Increases H2S HS- (1) Write a…

A: Since you have posted a question with multiple questions, we will solve first question for you. To…

Q: 15. The pka for o-fluorophenol is 8.81. Draw the predominant form in solution at the given pH…

A: Given information:pKa for o-fluorophenol = 8.81

Q: The pKa of benzoic acid is 4.2 Using henderson hasselbalch equaequation calculate the ratio of…

A: Given:: pKa = 4.2 pH = 7.9 ratio [R-COOH] : [R-COO-] = 1: ?

Q: Which of the following equations represents the acid equilibrium associated with Kaz for H3PO3? A)…

A: Given : To write the acid equilibrium associated with Ka3 for H3PO3.

Q: Phosphoric acid (H3PO4) is a triacid (pKa1 = 2.2 ; pKa2 = 7.2 ; pKa3 = 12.3). Write the balanced…

Q: Which of the following is false regarding the reaction below? H2SO3(aq) + H20(1) – HSO3 (aq) +…

Q: B. Identify the Bronsted-Lowry acid (loses an H- ion base agins an H. ion))conjugate acid, and the…

A: According to Bronsted-lowry concept of Acid-BaseAcid: Acid are those species that releases/ loses H+…

Q: What is the weight NaCH3COO of that must be added to 750.0 mL of 0.180 M acetic acid to form a pH =…

Q: At 25°C, what is the hydronium ion concentration ina. 0.200 M chloroacetic acid? b. 0.0200 M…

A: When the equilibrium is attained, the determination of species concentration can be done by ICE…

Q: When ammonium (NH4+) is placed in water, a chemical reaction occurs and an equilibrium is…

A: Given: The equilibrium is established when ammonium (NH4+) is placed in water: NH4+ (aq) + H2O (l) ⇄…

Q: Which of the following statements is FALSE? a. If acid HA has a lower pka than acid HX, then HX has…

Q: Bicarbonate reacts with water to produce carbonate ions and hydronium ions: HCO3 +H2O = CO2²- + H3O+…

A: According to Bronsted-Lowry theory, an acid is a proton donor and base is a proton acceptor. The…

Q: Describe the method to determine whether an amphoteric compound is acidic or basic given a table of…

A: In general, the pH of the acid is below 7. And pH of the base is above 7. A Higher Ka value…

Q: Which of the following will not act as a Bronsted base in water at 298 K, and not participate in…

A: Answer Which of the following will not act as a Bronsted base in…

Q: Assuming that base (B:) and acid (AH) are mixed in equal concentrations and using pka values of acid…

A: pKa for AH = 4.7 pKa = -log Ka Ka = 10-pKa Ka1 = 10-4.7 = 2×10-5 pKa for BH+ = 5.1 Ka2 = 10-5.1 =…

Q: Without reference to a pKa table, decide which compound in each pair is thestronger acid: a.) H2O or…

A: GIVEN: a.) H2O or HFb.) H2S or H2O

Q: The measured pH of a 0.1 M solution of HNO3 (a strong acid) is 1.0. If the measured pH of a 0.1 M…

A: Given data contains, Measured pH of 0.1 M solution of HNO3 is 1.0.

Q: Which of the following hydronium ion (H3O+) concentrations would produce a basic solution? a.…

A: The basic solution has a pH > 8.

Q: Complete the following table, which lists information about the measured acid dissociation constants…

A: Answer:- This question is answered by using the simple concept of calculation of pKa and ka using…

Q: The pH of a 1.0 M solution of pentanoic acid (HC;H,O2) is measured to be 2.42. Calculate the acid…

A: Given information: Concentration of pentanoic acid = 1.0M pH of pentanoic acid = 2.42 The…

Q: What is the Ka for a 0.1459 M acetylsalicylic acid solution, C9H7O4H, if it had a hydronium ion…

A: Using the the Rate constant expression at equilibrium we can find the rate dissociation…

Q: 1. During the first part of the mechanism in the reaction above, the catalyst forms a complex using…

A: For a hydrogen-bond complex, we have to identify the Lewis acid and Lewis base

Q: Formic acid(HCOOH) is a weak acid found in nature. The following represents the reaction for formic…

A: The Ka expression: In general it is given as shown below. Consider the general reaction Then,…

Q: Consider the reaction: H2SO3(aq) + H20(1) = HSO3 (aq) + H30 (aq) Identify the conjugate acid of the…

Q: Phosphoric acid reacts with water to yield dihydrogen phosphate ions and hydronium ions:…

Q: For a certain acid pK, = 5.88. Calculate the pH at which an aqueous solution of this acid would be…

Q: F. Each of the following reactions is displaced to the LEFT. Identify the stronger acid for each…

A: Ans. Strong acids order HSO4- > HC2H3O2 > H2S > HCO3-

Q: Identify the products of the second acid dissociation of H₃PO₄ in water.

A: Given :- H₂PO₄⁻(aq)+H₂O(l)⇌ To identify :- dissociation products of above given reaction.

Q: Identify whether the 3 strucutres in the attachment are lewis acid, lewis base, or either lewis acid…

A: Lewis bases are those species which have extra electron pairs present in the species and can donate…

Q: What are the products to the reaction depicted below, assuming that H2PO4 is the acid? H2PO4 H20 (1)…

A: The two reactions possible when H2PO4- reacts with water are stated below:

Q: A 0.200 M solution of diethylamine, a substance used in insecticides and fungicides, is only 3.9%…

A: Diethylamine((C2H5)2NH) is a weak base that dissociates in water as follows:…

Q: Identify the Bronsted-Lowry acid in the following reaction. H2O (l) + HCO31- (aq) → H3O+ (aq) +…

A: Given : H2O (l) + HCO3- (aq) → H3O+ (aq) + CO32- (aq)

Q: Calculate the percent ionization of benzoic acid at the following concentrations. (a) 0.14 M 4.0 2.2…

A: We need to calculate the percent of ionization for 0.00022 M benzoic acid . Ka value of benzoic…

Q: What is the [OH−] of 0.1763 M hydrazoic acid solution, HN3, if Ka = 1.9000e-5? HN3(aq) + H2O(l) →…

Q: Nursing Chemistry question drug name is Atorvastatin Lipitor formula C33 H35 FN2 O5 1. identify…

A: The drug given above is atrovastatin.

Q: Vitamin 'C' or ascorbic acid is an essential nutrient for human beings and certain other animal…

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

Given the reaction: HPO4 2- (aq) + HC2H3O2 (aq) ↔ H2PO4 - (aq) + C2H3O2 - (aq)

1. The acid in the forward reaction is _____________.
2. The acid in the reverse reaction is_____________.
3. The base in the forward reaction is______________.
4. The base in the reverse reaction is ____________.

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 : Introduction

VIEW

Step 2 : Explanation

VIEW

Step 3 : Conclusion

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps with 1 images

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

Classify each of the following substances into the appropriate category: 1 Lewis acid; 2 Lewis base; 3 substance that can act as either a Lewis acid or Lewis base; 4 substance that is neither a Lewis acid nor a Lewis base. a CCl4,b F, c Cu2+, d Fe3+, e O2
Calculate the percentages of dissociated and undissociated forms present in the following solutions: (a) 0.0010 M glycolic acid (HOCH2CO2H; pKa = 3.83) at pH = 4.50 (b) 0.0020 M propanoic acid (pKa = 4.87) at pH = 5.30
A triprotic acid (H3A) has pKA values of 3.08 (pKa1), 5.39 (pKa2), and 7.70 (pKa3). Which of the equalities is true when the pH is 4.24? Which of the equalities is true when the pH is 6.55? What is the predominant species of H3A at pH 3.85? What is the predominant species of H3A at pH 9.09?
When ammonium (NH4+) is placed in water, a chemical reaction occurs and an equilibrium is established as shown below. NH4+ (aq) + H2O (l) ⇄ NH3 (aq) + H3O+ (aq) The pKa of NH4+ is 9.25. Predict whether the acid form (NH4+) or the base form (NH3) is predominant at pH = 7.4. Explain your answer.
The pKa of NH4+ is 9.25. Predict whether the acid form (NH4+) or the base form (NH3) is predominant at pH = 7.4. Explain. Can you help me, please?
The pKa of NaH2PO4 is 6.86. Its conjugate base is Na2HPO4. One dissolves 5.0 grams each of NaH2PO4 and Na2HPO4 in 500.0 mL of water, how many grams each of NaH2PO4 and Na2HPO4 must be dissolved in enough water to make 1.0 L of solution whose pH = 7.2? If the final concentration of NaH2PO4 is 0.1 M.
In calculating pH by ICE method of 0.015 M CH2FCOOH (Ka CH2FCOOH = 2.6 x10-3), the change in CH2FCOOH can not be neglected because. a. Acid Dissociation constant, Ka, has a negative exponent. b. pH is not within +/- pka unit of pka of CH2FCOOH c. initial CH2FCOOH concentration is less than 0.1 M d. dissociation of [CH2FCOOH] will be more than 5% of initial [CH2FCOOH] ----------- To protect corrosion of materials made of iron, the surface of the iron material is electroplated with another metal. Given below information, which metal will be best to “galvanize” the material ? O2  + H2O + 2e- ->   4OH-(aq) .... E0 = 0.401 v Fe2+(g) + 2e- - ->   Fe ............ E0 =(-) 0.440 v Cu2+(g) + 2e- - ->   Cu ...........E0 = 0.337 v Ni2+(g) + 2e- - ->   Ni ............ E0 = (-)0.250 v Zn2+(g) + 2e- - ->   Zn ............ E0 =(-) 0.763 v a. Zn b. Ni c. Cu d. Fe2+ ------------ Given :  C (s) + H2O(g) <-> CO(g) + H2(g)       Which of the following will shift equilibria to form…
When ammonium (NH4+) is placed in water, a chemical reaction occurs and an equilibrium is established as shown below.   NH4+ (aq) + H2O (l)  ⇄  NH3 (aq) + H3O+ (aq) The pKa of NH4+ is 9.25.  Predict whether the acid form (NH4+) or the base form (NH3) is predominant at pH = 7.4. Can you help me, please?
When ammonium (NH4+) is placed in water, a chemical reaction occurs and an equilibrium is established as shown below.   NH4+ (aq) + H2O (l)  ⇄  NH3 (aq) + H3O+ (aq) The pKa of NH4+ is 9.25.  Predict whether the acid form (NH4+) or the base form (NH3) is predominant at pH = 7.4. Can you help me?
5,Calculate the [OH-]of the solution with pH=10.50 Group of answer choices 1.05 x 10-10 5.0 x 10-10 3.2 x 10-10 3.2 x 10-4 6, Use the Ka values for the following acids to find the strongest conjugate base: HSO4- 1.2 x 10-2H2PO4- 6.3 x 10-8HCO3- 4.7 x 10-11 Group of answer choices A, H3PO4 B, H2SO4 C, HPO42- D, H2CO3 E, CO32- F, SO42-
if the pH at one half the first and second equivalence points of a dibasic acid is 4.80 and 7.34, respectively, what are the values for pKa1 and pKa2?
The conjugate base that is produced after the first ionization step of carbonic acid when it has reacted with ethyl amine (CH3CH2NH2) would be _________. H2CO3 CH3CH2NH3+ HCO3- CO3-2 CH2CH2NH Given a Ksp of 4.96 X 10-9 for limestone (calcium carbonate), the calcium concentration in a limestone solution will be__________ the Ksp. greater than less than the same as cannot be determined