13.2) What is the pH of a 0.85 M solution of sodium hydrogen sulfite, NaHSO3 (Ka=6.0 x 10^-8)?

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: 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: In the laboratory, a general chemistry student measured the pH of a 0.345 M aqueous solution of…

A: The ionization reaction for caffeine is as follows, C8H10N4O2+H2O→HC8H10N4O2++OH- For above…

Q: The hypochlorite ion, ClO-, acts as a weak base. When ClO- acts as a base, which atom, Cl or O, acts…

A: To know which is the proton acceptor we see the valancy of the Cl and the O. In O there is two…

Q: -8 What would be the pH of a solution 5. The K, for hydroxylamine, HONH2, is 1.1 x 10 prepared by…

A:

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

A: Given: The compound is NaF.

Q: Vhat is the pH of a solution containing 0.2 M citric acid (pKa = 5.4) and 0.1 M sodium citrate?

A: Introduction: Since having sodium citrate that is a buffer solution so we can use the…

Q: In the laboratory, a general chemistry student measured the pH of a 0.453 M aqueous solution of…

A: The dissociation of acetic acid is given as, CH3COOH↔CH3COO- + H+ By definition, the acid…

Q: The hydronium ion concentration of vinegar is approximately 4 × 10−3 M. What are the corresponding…

A: Given : hydronium ion concentration i.e [H3O+ ] = 4 X 10-3 M

Q: Milk of Magnesia, a suspension of Mg(OH)2, a laxative, can be used as treatment for constipation…

A: We will first calculate solubility of Mg(OH)2 using Ksp ,then find grams of undissolved substance…

Q: The active ingredient in aspirin is acetylsalicylic acid (HC9H7O4), a monoprotic acid with a Ka of…

A:

Q: A student determines that the value of pK, for HCN = 9.26 . What is the value of K,? a

A: Given  PKa for HCN   = 9.26  Ka    = ?

Q: The ionization constant (Kb) of aniline (C6H5NH2) is 2.35 x 10–5. If 7.285 grams of aniline is…

A: We have to predict the equilibrium concentration of all species.

Q: Calculate the pH of a solution made by dissolving 1.87g of sodium caproate (NaC6H11O2) in water and…

A: We will calculate pH

Q: The pOH of an aqueous solution of 0.354 M acetylsalicylic acid (aspirin), HC9H7O4, is

A:

Q: What is the pH of a 0.620 M solution of Ca(NO2)2 (Ka of HNO2 is 4.5 x 10 4)?

A:

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

A:

Q: The pOH of an aqueous solution of 0.428 M acetylsalicylic acid (aspirin), HC9H7O4, is

A: Aspirin is a monoprotic weak acid with formula HC9H7O4. Hence it will dissociate partially as per…

Q: 5. The hydronium ion concentration of vinegar is approximately 4 x 10-³M. What are the corresponding…

A:

Q: HCIO is a weak acid (Ka 4.0 x 10-8) and so the salt NaCIO acts as a weak base. What is the pH of a…

A: Given data; Ka=4×10-8Also, Kw=Ka×KbAnd,Kw=1×10-14 Consider the dissociation of given weak acid as;…

Q: Discuss the justification for this statement: “Although one does not normally regard NH+4 as an…

A: An acid is the species which gives proton when present in an aqueous solution. The tendency of an…

Q: What is the pH of a 0.830 M solution of Ca(NO₂)₂ (Ka of HNO₂ is 4.5 × 10⁻⁴)?

A: The chemical equation may be written as: The given data is: Concentration of Ca(NO2)2 =0.830M Ka of…

Q: What is the pH of a solution when 2. 75 g of ammonium chloride, NH4CI, is used to make 100 cm3 of…

A: Number of Mole-ratio of given mass of substance to the molar mass of substance is called number of…

Q: ulate the pH of a solution prepared by dissolving 1.90 g of sodium acetate, CH,COONA, in 85.0 ml of…

A: Given, Mass of Sodium Acetate = 1.90 g Ka of CH3COOH is 1.75×10-5.

Q: What is the pH of 0.0100 M potassium phthalate (K2P)?

A: The acid ionization constant, Ka of potassium hydrogen phthalate (KHP) is 3.91×10-6. The dipotassium…

Q: A weak base, BOH, has a ph of 9.80 and Ka equal to 1.0 x 10-5. What is the Molarity of BOH?

A: Given data, The pOH of a weak base is calculated as shown below.

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

A:

Q: find the pH of the solution Ca (OH) 2, which is obtained when dissolving 0.5 grams of Ca (OH) 2 in 1…

A: We can find the concentration of Calcium hydroxide using moles and volume. Then we know we have…

Q: Given lead (I1) hydraxide Pb (OH),what is the molar solubility? K" 1.2x10 iwhat is the pH of this…

A: Since you have posted multiple questions, we are entitled to answer the first only.

Q: If the K, of a weak base is 3.9 x 10-6, what is the pH of a 0.48 M solution of this base?

A: Kb- is a dissociation constant of weak base. Formula is, pOH - pOH is defined as negative logarithm…

Q: The concentration of CH3COOH (pKa=4.75) in vinegar is about 1.0 M. With this what do you predict the…

A: pH is the negative logarithm of Hydrogen ion concentration. pH of a solution can be calculated as:…

Q: 2. If you make a solution by mixing 25.mL of 0.50 M acetic acid (CH3COOH) and 25 mL of 0.30 M sodium…

A: Given,  [CH3COOH] = 0.50 M  Volume of CH3COOH = 25 mL  [CH3COONa] = 0.30 M  Volume of CH3COONa = 25…

Q: CH;NH, is a weak base (Kp = 5.0 × 104), so the salt CH,NH,NO, acts as a weak acid. What is the pH of…

A: The pH of salt of strong acid and weak base can be calculated by  using formula

Q: The pOH of an aqueous solution of 0.313 M acetylsalicylic acid (aspirin), HC9H704-

A:

Q: What is the pH of a sodium acetate (NaCH3CO2) solution prepared by adding 0.820 g of sodium acetate…

A: Given: Mass of sodium acetate = 0.820 g Volume of water             = 100.0 mL Ka of acetic acid…

Q: The Kp of dimethylamine [(CH3)2NH] is 5.90×104 at 25°C. Calculate the pH of a 1.55x103 M solution of…

A: Given :  Concentration of (CH3)2NH = 1.55 × 10-3 M  Kb = 5.90 × 10-4  To calculate :-  pH of…

Q: Calculate the pH of a 0.100 M NaCH 3CO 2 solution. Ka for acetic acid, CH 3CO 2H, is 1.8 × 103.

A:

Q: The pOH of an aqueous solution of 0.591 M phenol (a weak acid), C,H5OH, is

A:

Q: What is the pH of 0.273 M trimethylammonium iodide, (CH3)3NHI? The Kb of trimethylamine, (CH3)3N, is…

A: Kb = 6.3 x 10-5

Q: The pH of a 0.55 M aqueous solution of hypobromous acid, HBrO, at 25oC is 4.48. What is the value of…

A: The concentration of HBrO solution = 0.55 M. pH of aqueous HBrO solution = 4.48.

Q: 1) Calculate the pH of a solution prepared by dissolving 1.00 g of sodium acetate, CH,COONa, in 57.0…

A: Given that : The mass of salt (sodium acetate) = 1.00 gm The concentration of acid (acetic acid) =…

Q: What is the pH of a 0.600 M solution of HSO, (Ka = 6.6 × 10°)? (Please show your answers with 3 sig…

A: pH of solution is equal to the negative logarithm of hydronium ion concentration. pH=-log(H3O+) Ka…

Q: The Ka of hypobromous acid, HOBr, is 2.6 x 10-9. Calculate the pH of a solu tion which is composed…

A: PH of acidic buffer can be calculated as follows

Q: Formic acid, which is a component of insect venom, has a Ka = 1.8 x 10. What is the [H30) in a…

A:

Q: HCIO is a weak acid (K. = 4.0 x 10-8) and so the salt NaCIO acts as a weak base. What is the pH of a…

A:

Q: A tablet of a common over-the-counter drug contains 200 mg of caffeine (C8H10N4O2). What is the pH…

A: Given mass of caffeine = 200 mg The given volume = 225 mL Kb = 4.1 x 10–4 pH = ?

Q: The ionization constant of lactic acid, CH3CH(OH)CO2H, an acid found in the blood after strenuous…

A: Given: The ionization constant of the lactic acid = 1.36×10-4 Mass of lactic acid= 20.0g Volume of…

Q: If the KbKb of a weak base is 1.6×10−6,1.6×10−6, what is the pH of a 0.18 M0.18 M solution of this…

A: Concentration of the solution is 0.18 M. Kb = 1.6 x 10-6 The Ka value is calculated by following…

Q: What is the molarity of a solution made by dissolving 3.4 g of Ba(OH)2 in enough water to make 450.…

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.