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. 11.48 E. 4.78

Q: A scientist dilutes 50.0 mL of a pH 5.85 solution of HCl to 1.00 L. What is the pH of the diluted…

A: Given data,pH=5.85Volume of HCl=50mL=0.050LDilution=1.0LKw=1.0×10-14

Q: What is the pH of a 0.0015 M solution of HBr?     5.65     You need the Ka value to answer this…

A: What is the pH of a 0.0015 M solution of HBr?

Q: What is the pH of a 0.00450 M HNO3 solution? A) 2.35 B) 3.52 С) 4.50 D) 11.65

A: We know that, pH of the solution can be expressed as negative logarithm of hydronium ion…

Q: Determine the pH of a. 0.23 M solution of NH4BR. Express your answer to 2 decimal places.

A: pH is a measure of acidity of the solution and it is equal to the negative logarithm of hydrogen ion…

Q: Find the pH of a solution prepared by dissolving 1.80 g of potassium hydrogen phthalate (204.221…

A: Given data,Mass of KHP=1.80gMolar mass of KHP=204.221g/molMass of Na2P=1.20gMolar mass of…

Q: The weak base, B O H, has a K b value of 3.9E-5. Calculate the pH of this solution if the…

A: Given: Kb of BOH = 3.9×10-5 Concentration of BOH = 0.706 M

Q: (3 points) The pH of a sample of soap solution is 10.80. Calculate its molar hydronium…

A: 4th option is correct. Solution is given in step no 2:

Q: Determine the pH of a 0.01462 M HNO3 solution.  Record your answer to 2 decimal places.

A:

Q: 3. Calculate the pH, [НЗО),[Он], к, and a values. 1.0 М 1.0 М pH [H3O`] [OH] 0.02 HCI Ка HCI pH 2.30…

A: Given : HCl : pH = 0.02 HC2H3O2 : pH= 2.30 NH3 : pH = 11.8

Q: 36. Determine the pH of 0.25 M HBr solution.* A. 0.30 O B. 0.52 C. 0.60 O D. 13.0

A: 1 mol of HBr contains one mole of each H+ and Br- ions each.

Q: 28. The pH of a solution is measured to be 10.4. What are the values of (HO] and (OH for this…

A:

Q: If a solution of hydrochloric acid has a hydronium concentration of 1.5 x 10-5 M, what is the pH?…

A: pH = -log[H3O+]

Q: Determine the pH of a 1.00×107 M aqueous solution of HBr. A 6.17 B 6.79 7.00 Your answer D 7.12

A: When solution is dilute then H+ from H2O is also considered. PH of acidic solution can't be 7 or…

Q: Calculate the pH of an a. 3.00 b. 4.00 с. 5.00 d. 6.00

A: Given, Ka = 4.9 x 10-10  PH = ?

Q: Calculate the pH of a solution of 0.100 M H2SO3. Ka1 = 1.23 x10-2 Ka2= 6.6 x 10-8

A: First dissociation                                                                2nd…

Q: Calculate the pH of 0.075 MNAOH. (a) 10.40(b) 11.12(c) 11.46(d) 12.88(e) 13.26 fhudrochloric acid is…

A:

Q: 40 Be sure to answer all parts. X 01:20:04 In the following equation, identify the acids, bases, and…

A:

Q: What is the pH of a 0.015 M HClO4 solution?   a. 12.18   b. 1.82   c. 0.030   d. 0.015

A: ph of 0.015 M HCLO4=?

Q: 2) Use the data below to answer the questions that follow substance milk Pickle juice Oven cleaner…

A: Given,  [H3O+] for milk = 3.2×10^(-7)  [H3O+] for pickle juice = 2.0 × 10^(-4)  [H3O+] for oven…

Q: What is the pH of a 0.0020 M HCl solution?   a. 11.30   b. 0.0020   c. 0.0040   d. 8.80   e.…

A:

Q: Find the pH of a solution prepared by dissolving 1.80 g of potassium hydrogen phthalate (204.221…

A: Given solution is an acidic buffer solution.   Treat mono salt as acid and di potassium salt as its…

Q: neutral ? II maintain its pH. Solution is acidic, basic, or neutral? [H3O+ ] [ОН-1 PH 4.56 x 10-2…

A:

Q: Solution X 100 mL of 0.10 M HCI Solution Y 200 mL of 0.50 M NAOH Solution Z 300 mL of distilled…

A: The solutions given are,

Q: The hydronium ion concentration of a solution is 5.03×10+-2 M what is the pH A) 0.0503 B) 0.702 C)…

A: [H3O^+] = 5.03 × 10^-2M

Q: Determine the pH of a 0.18 M solution of NaN3 (Ka for HN3 = 1.9 × 10−5)   a. 4.0 b. 9.0 c. 5.0 d.…

A:

Q: Calculate the pH of a solution that has an [H+1] equal to 9.21 x 10-10 M.  Enter your answer to 2…

A:

Q: 36. Determine the pH of 0.25 M HBr solution. * A. 0.30 B. 0.52 C. 0.60 O D. 13.0

A: • The values provided in the question are:-     i) Concentration of hydrobromic acid solution, [HBr]…

Q: Calculate the pH of a solution if the concentration of OH- is 2.67 x10^(-5) M A. 14 B. 4.57 C.…

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

Q: What is the pH of a 0.3M solution of Ba(OH)2? Select one: a. 0.22 b. 13.47 c. 0.52 d. 13.78

A: Given:- For a solution Ba(OH)2 , Conc = 0.3M pH = ?

Q: What is the pH of a 0.040 M HNO 3 solution? A. 1.40 B. 1.70 C. 0.040 D. 12.30

A:

Q: alculate the pH of a solution of 0.100 M Na2SO3. Ka1 = 1.23 x10-2 ; Ka2= 6.6 x 10-8 A. 4.55 B. None…

A: Sodium Sulphite (Na2SO3) is regarded as the fully deprotonated form (SO32-) of diprotic acid H2SO3.…

Q: A week diprotic acid H2A has Ka1 = 4.2 × 10–7 and Ka2 = 4.8 × 10–11. Determine the pH of a 0.17 M…

A: Ka1 = 4.2 × 10–7     pKa1 = 6.376 and Ka2 = 4.8 × 10–11    pKa2 = 10.319

Q: V. Milk of magnesia has a pH of 10.2. What is the [OH] of milk of magnesia? pH= 162 =) plO H)= 3.8…

A:

Q: What is the pH of a solution of 0.65 M Acetic Acid? Select an answer and submit. For keyboard…

A:

Q: 4) Calculate the [H+] in a solution with a pH of 9.88? a) 4.1 M b) 9.9 M c) 7.6 x 10^-5 M d) 1.3…

A: pH of the solution is 9.88

Q: Calculate the pH of 0.221 M HN0 3( aq). O a. 1.510 O b.-1.139 Oc. 2.210 O d. 0.656 O e. 13.779

A:

Q: I have 3.025 lb H2SO4 and 200 gal of water.  How many molecules of sulfuric acid do I have?  What is…

A:

Q: Methylamine (CH3NH2) has Kb = 4.4 x 10–4. What is the pH of 0.15 M aqueous solution of methylamine?…

A: Value of pH of a solution is used to measure acidity or basicity of a solution. At room temperature,…

Q: Calculate the pH of a 5.84×10^−5 M HCOOH solution with a Ka=1.76 x 10^−4…

A: Given:             HCOOH(aq)<-------------->H+(aq) + COOH−(aq) The molar concentration of the…

Q: Find the pH of a 0.011 M solution of HF. (The value of Ka for HF is 3.5×10−4

A: Given, initial concentration of HF= 0.011 M          and, Ka= 3.5 x 10-4 We know that, pH is equal…

Q: Chemistry Calculate the pH of 0.0035 M KOH. Note: You are starting with a base. 11.54 7.00 13.99…

A:

Q: The pH of 0.20 M HN03 is O a. 1.58 Ob. 0.70 C. 0.20 Od. 0.63

A: Using formula in these questions: PH = -log[H+] Where as [H+]-------> concentration of H+ Using…

Q: Calculate the pH of a 0.085 M solution of acetic acid, HC2H302. (ka=1.9x10-5) HC2H302 - H* + C2H3O2…

A: pH measures the strength of acids and base that how the solution is acidic and basic lower the pH…

Q: What is the pH of a 0.145 M solution of NaOH?   A. 13.16    B. 10.12   C. 11.16   D. 14.00

A: 1.  pH = - log [H3O+]       pOH = - log [OH-]       pH + pOH = 14

Q: Determine the pH of a 0.92 mol L–1 NaF solution at 25 °C. The Ka of HF is 3.5 × 10–5.     11.44…

A:

Q: What is the H,O"| of a solution of HI with a pH = 1.45? O la) 0.0355 O (b) 0.1173 O (c) 0.3548 O (d)…

A:

Q: What is the pH of a solution prepared by dissolving 20.26 g of NaOH (strong base) in enough water to…

A: First of all we have to calculate the concentration of NaOH, from which we get the concentration of…

Q: What is the pH of an aqueous solution at 25.0°C containing hydronium ions H+? Select one: a. 7.04…

A: To answer this question we have to know the pKw of water at 25.0 oC. The pKw at this temperature is…

Q: Determine the pH of 1.5 M HBrO. (Ka HBrO = 2.5 x 10–9)

A:

Q: Calculate the pH of 0.341 M HC2H3O2 (Ka of HC2H3O2 = 1.8 x 10 5) %3D Round to 2 decimal places. Your…

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.