Salts containing the phosphate ion are added to municipalwater supplies to prevent the corrosion of lead pipes. (a) Basedon the pKa values for phosphoric acid (pKa1 = 7.5 x 10 - 3,pKa2 = 6.2 x 10 - 8, pKa3 = 4.2 x 10 - 13) what is the Kbvalue for the PO43 - ion? (b) What is the pH of a 1 x 10 -3 M solution of Na3PO4 (you can ignore the formation ofH2PO4- and H3PO4)?

Q: A weak acid has Ka of 4.47 x 10-4.  What is pKa for this weak acid?

A:

Q: A 0.3654 g portion of pure formic acid (CH2O2, FW=46.03 g/mol, Ka=1.77 x 10-4) is dissolved in 50.00…

A: Given that, Mass of formic acid = 0.3654 g Molecular mass of formic acid = 46.03 g/mol Volume of…

Q: buffer solution is prepared from an unknown weak acid (HA) and its conjugate salt (NaA). If 500.00…

A: We will calculate pKa using henderson hasselbalch equation.

Q: Given aqueous solutions of 0.1 M weak acetic acid (CH3COOH, pKa=4.72) and 0.1 M sodium acetate…

A: Consider the volume of acetic acid in the final solution be x L and the volume of sodium acetate in…

Q: The following observations are made about a diprotic acid H2A: (i) A 0.10 M solution of H2A has…

A: pH of a 0.10 M solution of H2A is 3.10 and 0.10 M solution of a salt NaHA is acidic.

Q: 10.00 mL sample of 1.20 M HNO2 (analyte) (pKa = 3.34 and Ka = 4.57x10-4) is titrated with 1.20 M…

A: Given , pka = 3.34 Molarity of HNO2 = 1.20 M Volume of HNO2 = 10 mL Mmol of HNO2 = M × V   = 1.20…

Q: For CO2 in the atmosphere at 25 degrees C, kH = 3.4 x 10-2 mol L-1 atm-1 and the partial pressure of…

A: Given Data: Henry's constant, kH = 3.4 x 10-2 mol L-1 atm-1 Partial pressure of CO2 = 0.000405 atm =…

Q: 5) The oxides and hydroxides of gallium exhibit both acidic and basic behaviors B) What is pCa for a…

A: Gallium metal is stable in dry air. It gradually oxidizes in moist air to form a protective film…

Q: 14. What is the pH of a mixture of 0.20M acetic acid and 0.30M sodium acetate, if the pKa of the…

A: Dear student , since you have posted multiple questions we will allow to solve only first question…

Q: What is the pH of a 250.0 mL solution that contains 3.17 g of potassium monohydrogen phosphate and…

A: Given,  The pH of a 250.0 mL solution that contains 3.17 g of potassium monohydrogen phosphate and…

Q: The Ka of a weak acid is 3 x 10^-12 What is the pKa of this acid?

A: Ka which is dissociation constant of acid is given  3*10^-12  Pka = ?

Q: what do you predict the pH of vinegar tobe?

A: pH = -log[H+]  or  pH = -log[H3O+]

Q: The following observations are made about a diprotic acidH2A: (i) A 0.10 M solution of H2A has pH =…

A:

Q: What is the pH of a buffer that is 0.12 M in lactic acid [CH3CH(OH)COOH, or HC3H5O3] and 0.10 M in…

A: Buffer solution consists of mixture of weak acid and its conjugate base.

Q: Define pKa for a weak acid. What is the relationship between the value of the pKa and the strength…

A:

Q: 2. a. What is the ratio of H2PO4 to H3PO4 at a pH of3? Phosphoric acid, pKal =2.12, pKa2 = 7.21, and…

A: #2(a): H3PO4(aq) is a weak acid and H2PO4-(aq) is a conjugate base of the weak acid. Hence…

Q: Given a theoretical acid, HA, with a pKa of 6.52. Calculate the pH of 30.0mL of 0.400M HA, when it…

A: The total number of HA acids in the solution is determined below. nHA=MHA×VHA=0.400 mol/L×30.0…

Q: Which of the following is the best buffer at neutral pH (pH 7.0)? O Water, pKa = 14 Phosphoric acid,…

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

Q: What is the pH of a solution prepared by mixing 30.00 mL of 0.10 M CH 3CO 2H with 30.00 mL of 0.030…

A: The question is based on the concept of titrations.   we are titrating  a weak acetic acid with a…

Q: A beaker contains a total concentration of 0.73 molar of weak acetic acid with pKa = 5.55 and pH =…

A: We would show dissociation equation of acetic acid and write ICE table to calculate the…

Q: 6. a. Complete and balance the following acid-base reaction: H3PO4 (aq) + KOH (aq) → b. Calculate…

A:

Q: The pKa of lactic acid is 3.86. You have a mixture of lactic acid and sodium lactate, where the…

A:

Q: What will be the pH of a solution when 200ml of 0.1M HEPES in the basic form and 100mL of 0.1 M…

A: Given: Concentration of Base = 0.1 M volume = 200 mL = 0.2 L concentration of acid = 0.1 M volume =…

Q: A hypochlorous acid buffer is prepared with 0.10 moles HCIO and 0.10 moles CIO- and pH = pKa = 7.40.…

A: pH = pKa + log[salt]/[acid] ClO-  +  HCl  ----->  HClO  +   Cl- Number of moles of HClO formed =…

Q: Tris(hydroxymethyl)aminomethane [(HOCH,)3CNH, Tris or THAM] is a weak base frequently used to…

A: It is an example of a basic buffer solution. Molar mass of THAM is 121 g/mol

Q: 3. (a) How many grams of sodium succinate (140 g/mol) and disodium succinate (162 g/mol) must be…

A: A buffer solution of 50Mm with a pH 6, has to be prepared using sodium succinate and disodium…

Q: What is the pH of a solution made by titrating 265. mL of 0.014 M propanoic acid  (Ka = 1.34x10-5)…

A: Propanoic acid is the weak acid so pH of given titrating mixture is calculated as follows, Given.…

Q: How many grams of hyrogen phosphate and Sodil dinydrogen phosphate are heeded to make 100 mL of a…

A: Since you have asked multiple questions, we will answer only first question for you. In order to get…

Q: Phosphorous acid, H,PO,(aq), is a diprotic oxyacid that is an important compound in industry and…

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

Q: 2. The active component of aspirin is acetylsalicylic acid, HC,H,0., which has a K. of 3.0 x 10-4…

A: 2) Given: Ka of HC9C7O4 = 2.0 × 10-4  a) Given: Mass of HC9C7O4 = 0.500 g. And volume of solution =…

Q: A sodium hydrogen carbonate/sodium carbonate buffer system is to be prepared with a pH of 9.89.  The…

A: The question is based on the concept of buffer solution.   A buffer is a solution which resist any…

Q: Lactic acid, CH3CH(OH)COOH, is a monoprotic acid that is present in sour milk. The pH of a 0.100 mol…

A: [H3O+]= 10-pH [H3O+]= 10-2.44 [H3O+]=3.6308 x 10-3 M

Q: 30ml of 0.06M solution of protonated form of anion amino acid methionine (H2A+) is treated with0.09M…

A: Answer: Step 1: The amino acids have both acidic and basic groups. At high pH they behave like bases…

Q: 6. If 25.1 mL of 0.109M acid with a pKa of 5.27 is titrated with 0.108 M NaOH solution, what is the…

A: The volume of acid V1=25.1 mL The concentration of acid C1=0.109 M The strength of an acid is pKa =…

Q: The desired pH is 6.4 in creating a buffer system/buffer solution of about 50-60mL. Therefore, a…

A: A buffer solution is made of a weak acid and the salt of that weak acid. The pH of the buffer does…

Q: The pH of a solution containing 0.010 M lactic acid and 0.087 M lactate is 4.80. Calculate the pKa…

A: Given:Concentration of lactic acid = 0.010 M Concentration of lactate = 0.087 M  pH of the solution…

Q: Histidine has ionizable groups with pKa values of 1.8, 6.0, and 9.2, as shown below (His = imidazole…

A: The three pKa values shows that there are 3 replaceable hydrogens in the molecule(represented as…

Q: The Kb for ethylamine (C2H5NH2) is 5.6 x 10-4. What is the pH of a 0.020 M solution of ethaylamine?

A: The reaction is –              C2H5NH2 + H2O↔C2H5NH3+ + OH-I                 0.02…

Q: . The acetate buffer contains 0.200 M acetic acid and 0.0500 M sodium acetate. Given that the Ka of…

A: PH of buffer solution is calculated by using Henderson Hasselbalch equation

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

A: Solution a)

Q: Arrange the following acids in order of decreasing acid strength, 1 being the weakest and 4 being…

A: Ka is the dissociation constant of acid. Higher the value Ka, more is its dissociation so stronger…

Q: A 100 ml of 0.100 M phosphate buffer solution with a pH of 8.10 is to be prepared by adding 1.00 M…

A: The required pH of the buffer is 8.10, which is closest to the pKa2 value. H2PO4(aq) ⇌ HPO4-(aq) +…

Q: Sodium hypochlorite (NaOCl, the active ingredient of all bleaches) was dissolved in a solution…

A: pH of buffer solution is calculated by using Henderson Hassel balch equation

Q: What is the volume of HF(g) (ideal gas at 1 atm and 25°C) required to be bubbled into 250 ml…

A: HF is the conjugate acid of F-.

Q: Given that the Kf for [Ni(H2O)5(NH3)]2+ is 501 and Ka for NH4+ is 2.0 x 10-5, what is the…

A:

Q: FRQ1: Consider the titration of 25.00 ml of 0.08 M of a weak acid, HA, with 0.125 M NAOH. Calculate…

A: We are authorized to answer three subparts at a time, since you have not mentioned which part you…

Q: What is the pH of a buffer that is 0.12 M in lactic acid [CH3CH(OH)COOH, or HC3H5O3] and 0.10 M in…

A: The acid ionization constant for lactic acid is 1.4×10 -4.

Q: Calculate the pH of 0.65 M of a weak acid HA with Ka = 2.56 x 10 -6.      5.59     2.89…

A:

Q: A solution prepared by dissolving 2.25 g HA (MW = 51.0) and 4.00 g of NaA in 500 mL of solution has…

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.