What is the pH of 0.0050 HF (Ka = 6.8 x 10-4)?  11.27 2.30 2.73 11.70

Q: The diagram below represents a monoprotic acid, HA. If 14.75 mL 0.0200 M KOH are added to 32.47 mL…

A: The given acid is monocratic so it will give one proton and the given base KOH also give one…

Q: Q2// 1000 ml of o.1M hydrochloric acid were added to 1000 ml of o.1M ammonium hydroxide, ammonium…

A: Given that 1000 ml of 0.1 M hydrochloric acid and 1000 ml of 0.1 M ammonium hydroxide is reacted…

Q: Calculate the pH of a 3.80×10^−3 M HCl solution. a) 0.628 b) 3.39 c) 11.2 d) 2.42 e) 1.50

A: To find pH

Q: What is the pH of a solution with [H+] = 0.002M? Select one: a. 2.7 b. 0.3 c. 2.0 d. 1.3

A: Given: [H+] = 0.002M pH: The concentration of hydrogen ion is measured using pH scale. The pH of a…

Q: Morphine is a weak base with a Kb = 1.6 x 10-6. What is the pH of an 0.83 M solution of morphine?

A: Given data,Kb=1.6×10-6Molarity=0.83M

Q: 6. OH- concentration is 1.233x10(-7). What is the pH? 8.09 5.09 6.09 7.09

A: PH = -log [H+] POH= - log [OH-] Given [oH-]= 1.233×10-7

Q: The pH of an aqueous solution at 25.0 °C is 10.20. What is the molarity of H+ in this solution? A.…

A: pH = -log[H+] 10.20 = -log[H+] [H+]=10-10.22        = 6.30×10-11 M

Q: 4 Determine the pH a 0.60 M NH&CI solution. NHẠCI (aq) + H20 (1) = H30*(aq) + NH3(aq) Ka = 5.56 x…

A:

Q: the pH of a certain solution is 4.25. what is the hydroxide ion concentration of that solution?…

A: We have given that  The pH of certain solution is 4.25 what is the hydroxide ion concentration of…

Q: Acetic acid (HC2H3O2) is a weak acid (Ka = 1.8 x10-5). Calculate the pH of a 10.6 M HC2H3O2…

A: Dissociation of acetic acid and pH calculation

Q: 3. The Kb value of Ethylamine (C2H5NH2) is 5.9 x 10-6. The pH of 0.10 M Ethylamine aqueous solution…

A:

Q: 1. What is the pH of a neutral solution at 37°C, where Kw equals 2.5 x 10-14 (a) 7.00 (b) 6.80 (c)…

A: In this question, we want to determine pH of the neutral Solution.  How we can determine pH for this…

Q: Determine [OH ], H*, and the pH of each of the following solutions. а. 1.9 М CSCI [OH] = M [H*] =|…

A:

Q: Calculate the pH of a 2.0 M Ca(OH)2 aqueous solution. a. 13.4 b. 14.3 c. 14.6 d. 13.7

A:

Q: What is the pH of 0.1000 M Na₂HPO4? (K₁2=6.2x10-8, K3=4.8x10-13) What is the pH of 0.1000 M Na3PO4?…

A: The solutions considered are 0.1000 M Na2HPO4 and 0.1000 M Na3PO4. The question requires to…

Q: The pH of a 0.150 M aqueous solution of ammonium bromide (NH4Br) falls within what range?     2…

A: The concentration of ammonium bromide (NH4Br) = 0.150 M

Q: What is the pH of a 0.100M NH3 solution? Kb for NH3 is 1.8 x 10-5? NH3(aq) + H2O() = NH4+(aq) +…

A: NH3 is a base and NH4+ is its conjugated acid. pKb of ammonia is 1.8×10-5. The dissociation of NH2OH…

Q: Hydrogen lon Concentration pH Basic/Acidic 1.0.0015 2. 5.0x109 3. 1.0 4. 1.0x10-12 5. 0.0001 6. 1.00…

A: The pH of a solution is calculated by taking negative log of the concentration of hydrogen ions.  If…

Q: What is the pH of a 0.85 M H2SO4?   Show your ICE table and calculations.  Ka1 for H2SO4 is a very…

A: The sulfuric acid completely disassociates in the solution, hence we can assert that the…

Q: What is the pH of a 0.300 M NH 3 solution that has Kb = 1.8 x 10 ? The equation for the dissociation…

A: The pH of solution can be calculated as follows

Q: Calculate the pH of a 6.0 × 10–3 M KOH solution.   1.22 11.78 2.22 10.78 12.78

A: The pH of the solution can be calculated by using the formula given below as; pOH=-log OH-…

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: 13. What is the pH of a 0.0 1 5M Ca(OH)2 solution? a. 1.52 b. 12.18 c. 12.48 d. 1.82

A: The required equation is given below.

Q: 16. At 50°C, the Kw is 5.47 x 10-14. At this temperature, pure water A. is neutral. B. is slightly…

A: Hydroxide and hydroxyl ion are equal in amount    hence PH and POH are same hence solution is…

Q: What is the pH of a 0.25 M F- solution (Kb = 1.4 x

A: Given,   Concentration of Base = 0.25 M Kb = 1.4 ×10-11 pKB = -Log(Kb)   = -log(1.4×10-11) = 10.85

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: Carbonic acid, H 2CO 3, is a diprotic acid whose Ka1 = 4.3 x 10 -/ and K a2 = 5.6 x 10 -11.…

A: The dissociation reaction for H2CO3 is as follows : H2CO3-------------> H+ + HCO3^- calculate Ka1…

Q: What is the pH of 0.1M Na2HPO4. if,  pk1=4,   pK2=7,  pK3=11?

A: What is the pH of 0.1M Na2HPO4. if,  pk1=4,   pK2=7,  pK3=11?

Q: What is the pH of a 0.015 M solution of aqueous Ba(OH)2?

A:

Q: Calculate the pH of a 0.18 M solution of KNO2. (Ka (HNO2) = 4.5 x 10-4) Group of answer choices…

A: Given : Concentration of KNO2 = 0.18 M And Ka of HNO2 = 4.5 X 10-4  Since KNO2 is a completely…

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: Acetic acid (HC2H3O2) is a weak acid (K = 1.8 x10-5). Calculate the pH of a 17.6 M HC2H3O2 solution.…

A: An acid dissociates into proton and a negatively charged molecule in equilibrium. It can be shown in…

Q: What is the pH of 8.3 x 10-3 M HC1? pH =

A: Dear student since you have asked multiple questions but according to guidelines we will solve 1st…

Q: . Calculate the pH of .01 M NaOH A. 12 B. 2 C. 14 D. 1   2. Calculate the pH of .01 M HCI  A. 2 B. 1…

A:

Q: Calculate the pH of a 1.7 M Ca(OH)2 aqueous solution. a.13.8 b.14.5 c.13.5 d.14.2

A:

Q: What is the pH of a solution that is 1.67x10-5M H+?a. 4.8b. 5.2c. 0.22d. 10.2

A: According to question,  Concentration of H+ ion is = 1.67* 10-5

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: What is the pH of an aqueous solution at 25.0 °C in which [OH−] is 0.0050 M? A. 11.70 B. -2.30 C.…

A: The pH of any solution is given by  pH = -log[H+] = 14 + log[OH-]  where [OH-] = concentration of…

Q: Ascorbic acid (vitamin C, C6H;O6) is a diprotic acid (Ka1 = 8.0x10 and Ka2 = 1.6×10-12). What is the…

A:

Q: What is the pH of a 1.00*10-°M solution of KOH at 25 °C? 5.000 9.000 12.400 13.980 7.004

A: pOH= -log[OH-] = -log 10-9 = 9

Q: Calculate the pH for the following concentration: [H,0*] = 2.19 x 10-5 M A. pH=4.7 B. PH=4.9 C.…

A:

Q: A solution whose pH is equal to 4.0 has a hydrogen ion concentration of _____.  (A)1 x 104 M (B)1 x…

A: The pH of a substance is given by, pH = -log[H+]

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: Arrange the following solution from lowest pH to highest pH: a) 0.20 M CH₃COOH (Ka = 1.8 x 10⁻⁵),…

A: (a) First of all First of all the ICE table has to be drawn for the dissociation of acid as:…

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: What is the pH of an aqueous solution at 25.0 °C that contains 3.98 × 10-9 M hydronium ion? A)…

A: Given : Hydronium ion concentration = [H3O+ ] = 3.98 X 10-9 M

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: [H3O+] = 9.645 x 10-3, calculate the pH:

A: Given Data :-     Concentration of H3O+ ion          [ H3O+] = 9.645 × 10-3

Q: What is the pH of an aqueous solution at 25.0 °C in which [H+] is 0.0030 M? A. -5.81 B. 2.52 C.…

A: pH is the measure of acidic or basic nature of the aqueous solution of a substance. The pH of the…

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.