B represents an acid-base indicator and behaves like a base. Its dissociation equilibrium in an aqueous solution can be written as:

Q: Phenylacetic acid (C6H5CH2COOH, simplified here as HPAc) builds up in the blood of persons with…

A: Answer: Given data: pH=2.62α=0.02C=0.12M

Q: Write the Lewis structures of the reactants and product of each of the following equations, and…

A: (a)

Q: Boric acid, BOH is used as a mild antiseptic. What is the pH of a 0.025 aqueous solution of boric…

A: Ka= [product]÷[Reactant] Then take assumption degree of ionisation is very Very less than 1

Q: A solution of sodium chlorite is prepared using 0.38 mol L1 NaOH as the solvent. The pK, of chlorous…

A: Solutions- Given- NaOH Conc. = 0.38 mol/lit, pKa of chlorous acid = 2, conc. of sodium chlorite =…

Q: For a weak acid (CH3COOH) that is titrated with a strong base (NaOH), what species (ions/ molecules)…

A: The stoichiometric point is also known as the equivalence point. It is the point when the complete…

Q: The pH of an aqueous sodium fluoride (NaF) solution is __________ because __________   7; sodium…

A: Given: The compound is NaF.

Q: The useful pH range for a typical indicator is ________ 14 2 4…

A: pH is also called as the power of H+ ions. The pH value tells us about the acidic or the basic…

Q: Write a net ionic equation for the overall reaction that occurs when aqueous solutions of oxalic…

A: Oxalic acid (H2C2O4) is a diprotic acid. To neutralize 1 mole of H2C2O4, we need 2 moles of NaOH.…

Q: Acid strength decreases in the series HI > HS04 > HF > HCN. Which of these equal molar salt…

A:

Q: Consider the following reaction and that H2CO3 is a weak acid, H2CO3 + H2O ==== HCO3- + H3O+. If…

A: Acid can be defined as a species that give hydrogen ions in solution. Acid can be weak or strong on…

Q: If a buffer solution is 0.170 M in a weak base (Kb = 4.2 × 10-5) and 0.490 M in its conjugate acid,…

A: Buffer solution: It is an aqueous solution which contains a mixture of a weak base and its conjugate…

Q: K, of a weak acid HX is 2.16 x 10-6. During a titration, an analyte solution containing a mixture of…

A: The Henderson Hasselbalch equation is given by, pH = pKa + logsaltacid where Ka is the acid…

Q: Lactic acid, HC3HSO3, is a weak acid and found in sour milk. The conjugate base of Lactic acid is…

A: Calculation of Ka value of lactic acid:  The concentration of sodium lactate NaC3H5O3 = 0.089 M The…

Q: 2.1 The correct indicator was added to 25.00 mL of a 0.1340 M solution of pentanoic acid…

A: Pentanoic acid is a weak organic acid. Its Ka is 1.4 x 10-5.  Its concentration is 0.1340 M and…

Q: A 245.0 mL sample of 0.15 M Ba(OH)2 is added to 438. mL of 0.20 M HNO3. What is the pH of the…

A:

Q: How many mL of a 5.0-M solution of sodium borate must be added to a 200-mL solution of 50 mM boric…

A: Pka of boric acid = 9.14    Cl+ consider x ml  5.0 M sodium borate is  required.   PH  = Pka +…

Q: Certain metal cations can act as Lewis acids in water to produce an acidic solution even though the…

A: Here Co2+ will react with water to release H+ ions. Thus it remains as, Co2+ + 2 H2O --->…

Q: In the laboratory, a general chemistry student measured the pH of a 0.509 M aqueous solution of…

A:

Q: Acid strength decreases in the series HI > HSO4 > HF > HCN. Which of these equal molar salt…

A: Solution: We know as pH increases basic nature of compound increases. The pH of any salt depends on…

Q: Calculate the pH of a solution containing a salt B Cl derived from a strong acid (HCl) and a weak…

A: The concentration of hydrogen ion in the salt solution is calculated as shown below where C is the…

Q: At 22 °C, an excess amount of a generic metal hydroxide, M(OH),, is mixed with pure water. The…

A:

Q: Fill in the left side of this equilibrium constant equation for the reaction of carbonic acid…

A: in this question given ka ka= Acid dissociation constant, acid dissociation constant is used to…

Q: Consider the generic dissociation equation... HA + H20 H3O* + A° .where HA is a weak acid Based on…

A: Buffer Solution is a water-based solution that consists of a mixture of a weak acid and its…

Q: a Consider sodium acrylate, NaC3 H3O2. K, for acrylic acid (its conjugate acid) is 5.5 x 10-. Write…

A:

Q: Calculate the pH at equivalence. The p K of nitrous acid is 3.35.

A:

Q: When 25.0 mL of 0.400 M hydrobromic acid and 25.0 mL of 0.400 M potassium nitrite are combined, the…

A: Given that: the volume of hydrobromic acid= 25.0 mL = 0.025 L molarity of hydrobromic acid= 0.400 M…

Q: Thymol blue is a unique indicator that has two set of color change, red to yellow near pH = 1.5 and…

A: There are different color indicators that are available for the determination of the endpoint of a…

Q: The acid ionization constant for a certain monoprotic acid (HA) is 1.57×10−4. What is the pH of a…

A:

Q: If a buffer solution is 0.140 M in a weak base (Kb= 1.8*10^-5) and 0.590 M in its conjugate acid,…

A:

Q: ACID-BASE EQUILIBRIA Doc Jill wants to determine the Ao of a weak acid she isolated called…

A:

Q: Select the chemical equation that represents the most important process impacting pH after…

A: Sr(C2H3O2)2 is a salt .Thus it dissolved in aqueous solution and ionizes .

Q: Why does an indicator change from its acid color to its base color over a range of pH values? In…

A: indicators are the substance whoose solution changes colour due to Changes in PH. These are called…

Q: The acid constants of the polyprotic acid НЗASO4 are К_a1 %3D 5х10 ^-3, К_а2 - 8х10^-8, К_а3 %3D…

A:

Q: The images below represent solutions of two acids, HX and HY. (H2O is omitted for clarity.) Which…

A: Weak acid is partially ionized while stronger acid is completely dissociated into ions.  As HX is…

Q: value

A: When water is self ionized then water and it's ion present in equilibrium so that we used…

Q: ACID-BASE EQUILIBRIA Doc Jill wants to determine the Ao of a weak acid she isolated called…

A: Answer: When a weak acid is added into the water, its partial ionization takes place which causes…

Q: What is the pH for a weak monoprotic acid if a 0.020 M solution of the acid has a Ka of 3.28 x 10-7…

A: The H3O+ concentration for the weak acid is determined given below:

Q: 2.  The ionization constant for acetic acid is 1.8 x 10-5. How many grams of NaC2H3O2 must be added…

A: The Henderson Hasselbalch equation for acidic buffer is given as :

Q: what is the value of k for the reverse reaction if K forward + 6.49 x 10^-2

A: Answer

Q: The following reaction occurs: HNO,(aq) + NaOH(aq) → NaNO,(aq) + 2 H,0(1) Identify the correct…

A: When strong acid react with strong base neutralization takes place. (NaNO3 neutral salt) At…

Q: What is an acid–base indicator?

A: As per our guidelines,  you have posted multiple questions we can only answer first one.

Q: The value of K, at 25°C for proplonic acid (CaisCOgH) is 1.34 x 10. What is the pH of a 0.02019M…

A: Answer: This question is based on the understanding of Henderson-Hasslebalch equation that we use…

Q: ris(hydroxymethyl)aminomethane, commonly called TRIS or Trizma, is often used as a buffer in…

A:

Q: For a 0.00533 M solution of sodium benzoate, NaC6H5CO2, do the following. Identify the major species…

A:

Q: ACID-BASE EQUILIBRIA Doc Jill wants to determine the Ao of a weak acid she isolated called…

A: Since you have asked multiple questions questions, we will solve the first four question for you. If…

Q: One characteristic of blood that we rarely give a thought to is its pH. The pH of blood must be held…

A: Buffer is a solution that resists the change in its pH when small amount of acid or base is added to…

Q: Certain metal cations can act as Lewis acids in water to produce an acidic solution even though the…

A:

Q: In some natural systems the pH must be maintained within very narrow limits. e.g. in human blood the…

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…

Q: Boric acid, BOH is used as a mild antiseptic. What is the pH of a 0.025 aqueous solution of boric…

A:

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.