A tablet containing 500.0 mg of aspirin (acetylsalicylic acid or HC gH 70 4) was dissolved in enough water to make 100 mL of solution. Given that Ka = 3.0 x 10 4 for aspirin, what is the pH of the solution? O 2.54 3.52 O 5.08 O 1.57

Q: What is the pH of a 0.350 M solution of HF (Ka = 6.8 × 10⁻⁴)?

A:

Q: What is the pH of a 0.40 M ammonia solution? Ka is 5.6 X 10-10 11.43 O 2.57 O 9.18 O 4.82

A: Ka = 5.6 x 10 —10

Q: Determine the pH of a solution that is prepared by dissolving 4.6 g of Ba(OH)2 in 3.3 L water at…

A: Number of moles (n) of solute present in 1 litre solution is called " Molairty (M) " M = n / V (in…

Q: Carbonic acid, H2COS is a diprotic acid with Ka1 = 4.3 x 10 7 and Ka2 = 5.6 x 10 11. What is the pH…

A: Answer

Q: What is the pH of a 0.0470 M solution of methylamine (CH&NH2, Kb = 4.4 x 10 4)?

A: Calculate the hydroxide ion concentration released by methylamine. OH- = KbCOH- = 4.4 × 10-4 ×0.047…

Q: Calculate the pH of a 0.25M aqueous solution of sodium fluoride, NaF. (Ka = 6.7 x 104)

A: Given; Concentration of sodium fluoride (NaF) solution = 0.25 M Ka = 6.7 × 10-4 pH of the solution =…

Q: What is the pH of a 0.0270 M solution of hydrocyanic acid, HCN (Ka = 4.9 × 10⁻¹⁰)?

A: HCN is a weak acid , it ionizes  as follows  HCN <----> H+ + CN- Given , Concentration of HCN…

Q: Calculate the pH of the solution resulting from the addition of 20.0 mL of 0.100 M NAOH to 55.0 mL…

A:

Q: What is the pH of a 0.0730 M solution of methylamine (CH₃NH₂, Kb = 4.4 × 10⁻⁴)?

A: Given :- concentration of methylamine solution  = 0.0730 M  Kb for methylamine = 4.4 × 10-4  To…

Q: What is the pH of a 0.0650 M solution of methylamine (CH₃NH₂, Kb = 4.4 × 10⁻⁴)?

A:

Q: A sample of potassium acetate, KCH3CO2 (M=98), of mass 4.9 g is used to prepare 500 mL of solution.…

A: Answer: option b. 8.87 is the pH of the solution.

Q: What is the pH of a 0.0490 M solution of methylamine (CH₃NH₂, Kb = 4.4 × 10⁻⁴)?

A:

Q: Determine the pH of a solution made by adding 13.12g of hypochlorous acid (HCOL, MW-52.46 g/mol,…

A:

Q: What is the pH of .15 M KBRO(aq)? O 3.07 O 4.75 O 13.18 O 9.25 O 10.93

A:

Q: What is the pH of a 0.193 M w. acid HA solution? Ka = 6.61 x 10−6?

A: The acid is weak so it weakly dissociates in the solution. That is it gives an H+ ions slowly in to…

Q: What is the pH in a 0.0320 M aqueous solution of formic acid (HCOOH)? (For HCOOH, Ka=1.8 x 10–4)

A: HCOOH is a weak organic acid. It dissociates into formate ions and hydrogen ions. The ICE table for…

Q: Carbonic acid, H₂CO₃ is a diprotic acid with Ka1 = 4.3 × 10⁻⁷ and Ka2 = 5.6 × 10⁻¹¹. What is the pH…

A: pH of a 0.48 M solution of carbonic acid = 3.35

Q: Propionic acid, CH3CH2COOH, has a Ka = 1.34 x 105. If 10.00 mL of 0.080 M propionic acid is mixed…

A:

Q: Determine the pH of a solution that is prepared by dissolving 7.4 g of Ba(OH)2 in 8.7 L water at…

A:

Q: What is the pH of a 0.150 M solution of acetic acid (pKa=4.75) at 25 degree celsius?

A: Given, the concentration of acetic acid =0.150 Mand pKa of acetic acid =4.75 at 25 °Cwe are asked to…

Q: Calculate the pH of a 3.97×10³ M solution of NaF, given that the Ka of HF = 6.80 x 10-4 at 25°C.

A:

Q: What is the pH of a solution at 298 K that is prepared by diluting 275 mL of 0.551 M Ca(OH)2 to 2.50…

A:

Q: 3. Calculate the pH of a solution containing 0.10 M H3BO3 and 0.18 M NaH2BO3 Ka = 5.81 X 10 10

A:

Q: Milk of magnesia is a suspension of magnesium hydroxide in water. Although Mg(OH)2 is relatively…

A:

Q: What is the pH of a 0.0930 M solution of methylamine (CH₃NH₂, Kb = 4.4 × 10⁻⁴)?

A:

Q: 5. A 0.15 g Ca(OH)2 (MM = 74.092 g/mol) is dissolved in enough water to make a 0.500 L solution.…

A: Given, The mass of Ca(OH)2=0.15 g. The molar mass of Ca(OH)2=74.092 g/mol The volume of the…

Q: Carbonic acid, H₂CO₃ is a diprotic acid with Ka1 = 4.3 × 10⁻⁷ and Ka2 = 5.6 × 10⁻¹¹. What is the pH…

A: The carbonic acid is a diprotic acid. The major release of hydrogen ions occurs in the primary…

Q: Calculate the pH for a 10.0 M solution of NH3 (kp= 1.8x105) NH3 - NH4 + OH a 13.987 O b .013 O c…

A:

Q: What is the pH of a 0.0310 M solution of hydrocyanic acid, HCN (Ka = 4.9 x 10-10)?

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

Q: What is the pH of a solution prepared by dissolving 0.075 mol of Ba(OH)2 in water to give 455 mL of…

A:

Q: Calculate the pH of a 0.0101 M aqueous solution of formic acid (HCOOH, Ka = 1.8E-4). pH =

A: For weak monoprotic acid ( HCOOH) : pH = 0.5 x (- log Ka - log C ) pH = 0.5 x ( - log 1.8 x 10-4 -…

Q: What is the pH of a 0.0360 M solution of hydrocyanic acid, HCN (Ka = 4.9 x 10-10)?

A:

Q: 9) Calculate the pH of 1.5 M solution of hydroxylamine, NH2OH, at 25°C. К, 3D 9.1 х 10

A:

Q: What is the pH of a 0.21 M solution of methylamine

A: Given :-  Initial concentration of CH3NH2 solution = 0.21M  Kb = 4.4 × 10-4  To calculate :-  pH of…

Q: What is the pH of a solution prepared by dissolving 0.450 mol of NH3 in sufficient water to make…

A: Given,  The pH of a solution prepared by dissolving 0.450 mol of NH3 in sufficient water to make…

Q: Calculate the pH of a 0.20 M solution of NH4NO3. (Kb(NH3) = 1.8 x 10)

A: Salt of Weak base and Strong acid  pH = 7 - 1/2 ( pKb  - logC )

Q: Assuming 0.1 M concentrations, arrange the following acid solutions in order of increasing pH.…

A: Concentration of each given acid = 0.1 M (c) We know that -> [H+] = √(Ka ×c)

Q: Calculate the pH of a 0.10 M solution of sodium acetate (NaCH3COO) given that the Ka of acetic acid…

A:

Q: What is the pH of a 0.0570 M solution of hydrocyanic acid, HCN (Ka = 4.9 x 1010)? %3D

A: HCN is a weak acid. Hence it will dissociate partially as per the reaction HCN -----> H+ + CN-

Q: What is the pH of a 0.15M solution of potassium nitrate? (The Ka value for nitrous acid is 4.0 x…

A: Considering the given solution to be 0.15 M potassium nitrite, we have solved further.

Q: What is the pH of a 0.0670 M solution of methylamine (CH3NH2, Kb = 4.4 x 104)? %3D

A:

Q: Determine the pH of a solution that is prepared by dissolving 8.7 g of Ba(OH)2 in 2  L water at…

A:

Q: What is the pH of a 0.100 M  solution of sulfurous acid? Given: Ka1 = 1.70×10–2, Ka2 = 6.20×10–8

A:

Q: What is the pH of a solution of 0.0745 M NACH3O2 ? Ka = 1.8 x 10

A: Given: Concentration of NaC2H3O2, [NaC2H3O2]= 0.0745M Ka = 1.8 x 10-5

Q: Calculate the pH of 0.17 M propanoic acid CH3CH2COOH, found in the sample analysis of sewage water.…

A: We have CH3CH2COOH →CH3CH2COO- + H+ Concentration of propanoic = 0.17 M  Ka=1.3 x 10-5

Q: Calculate the pH of a 0.50 M solution of ammonia (NH3, Kb = 1.8 x 10P.) A. 9.22 B. 2.52 C. 9.26 D.…

A: It is known that ammonia is a weak base in its aqueous solutions. The dissociation reaction in the…

Q: Formic acid, HCOOH, has Ka= 1.8 x 10–4. Calculate the molar concentration of H3O+ in 0.15 M HCOOH…

A: using given value of ka and concentration  use equaction- H+=cα α=kaC use this boh calculate the…

Q: Write the balanced NET IONIC equation for the reaction that occurs when nitri acid and sodium…

A: The explanation is given below-

Q: 7. Determine the [H:O"1 concentration and whether the solution is acidic, basic, or neutral for: a.…

A: • We know,   • PH = 7 means Neutral.   • PH > 7 means Basic.   • PH < 7 Acidic.• H3O+ OH = Kw…

Q: Calculate the pH of a 6.71 x102 M NaOH solution 1.17O 2.17O 6.710 12.83O

A:

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.