the pH of a solution of 15 g NH4Cl and 15 g of NH3 in a 850mL solution? The Kb for NH3 is 1.8 x 10-5

Q: 0.10 mole of HCl is added to 1.0 L of 0.25 M NH3 solution.  What is the pH?  Kb for ammonia is 1.8 x…

A: Molarity is defined as total number of moles of solute present in 1000 ml of solution Molarity =…

Q: If we have a solution of weak acid HA (Ka = 1,00 * 10-6) and at pH 4,00. How much water needs to be…

A: Hey, as the volume of weak acid is not given in the question, I consider it as 25 mL in order to…

Q: 8. What is the PH of a solution with [H*]=1 x 10-³M ]3 2HCNO ]-3HF |-2 ]None of the others 9. What…

A: Hello. Since more than one question has been asked, the first question shall only be answered in…

Q: What is the Ph of a 0.23 M triethylamine (C2H5)3N solution? Kb for triethylamine is 5.3 x 10^-4.…

A: pH = -log [H+] pOH = -log [OH-] Also pH + pOH = 14

Q: What is the pH of an acetic acid solution (HC2H3O2) with concentration 0f 0.100 M. Ka=1.75 x 10-5 A.…

A: An ICE table is constructed to determine the equilibrium concentration of H3O+ as follows,

Q: Calculate the pH for an aqueous hydroiodic acid solution that contains 3.15 x 10^-3 hydronium ion.…

A: pH is the negative logarithm of Hydrogen ion (hydronium ion) concentration. It stands for power of…

Q: What is the resulting pH of a solution at 298 K made by mixing 50.0 mL of 0.355 M HCl and 25.0 mL of…

A:

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: The Kw value that we use for water is for room temperature (25°C). Calculate the equilibrium…

A:

Q: Strong Bases; Calculate pH [base] [H3O"] pH Step 1 The strong base dissociates completely in aqueous…

A:

Q: 5. Value for Kw at 50.00°C is 5.470 x 10-14. Calculate the pKwat 50.00°C. 6. Value for Kw at…

A:

Q: The value for Kw at 0.0°C is 1.14 x 10^-15. Calculate the pH for a neutral solution at this…

A: pH of a  solution is measure  of acidity or  of basicity of a solution

Q: Caculate the pH of a solution prepared by mixing 84.7 mL of a 0.25 M aqueous aniline solution…

A:

Q: What is the pH of a grapefruit that contains 0.007 M citric acid solution (C6H8O7)?   C6H8O7(aq) +…

A:

Q: Calculate the pH of 0.05 M Ba(OH)2 Group of answer choices 1.3 2.6 1.0 13

A:

Q: Y Part A pH= 420864 Hd 951 ΑΣΦ 14 3 12 10 20 What is the pH at the equivalence point? Express the pH…

A: Given titration curve:

Q: Name: 1. Determine the pH and pOH (to two decimal places) for each: (a) Pure water at 50 °C (Kw =…

A: Water undergoes self ionisation in the following manner- 2 H2O ↔ H3O+ + OH- The equilibrium constant…

Q: What is the concentration of a hydrosulfuric acid solution with a pH of 2.34? Group of answer…

A:

Q: What is the pH of a 0.15 M HOCl solution (Ka = 3.0 x 10-8)

A: HOCl is weak acid hence it dissociated less in solution

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: at 95 ℃ water has an autoionization constant (Kw) of 4.518 X 10-13. Determine the ph of pure water…

A: Given :- Kw at 95°C = 4.518 × 10-13  To determine :- pH of pure water at 95°C

Q: A generic weak acid was prepared and has a concentration of 0.471 M. Its Kb value is 4.91x10-10.…

A:

Q: Calculate the pH of 100.00mL of 0.15 M HF solution after 131.00 mL of KOH 0.15 M have been added. Ka…

A:

Q: The kw for water is 5.5 x 10-14 at 50oC.  What is the pH of a neutral aqueous solution at 50oC?…

A:

Q: Determine the pH of a 1.30 M solution of CH3COOK. Ka(CH3COOH) = 1.8×10-5 Express your answer to

A: 1- First Calculate the OH- ion concentration :  CH3COO- + H2O <------> CH3COOH + OH-   The…

Q: What is the pH of a 0.150 M NH4Cl solution? Kb of NH3 = 1.76 × 10−5

A: Given: Concentration of NH4Cl = 0.150 M Kb for NH3 = 1.76×10−5

Q: What is the pH of an aqueous solution at 25.0 °C that contains 1.35 × 10-8 M hydronium ion? Group of…

A: Given that, [H3O+] = 1.35*10-8 M pH = ?

Q: a solution is made from 0.23 M CH3NH2 (a weak base) and 0.24 M CH3NH3Cl. what is the pH of the…

A: The pH of this buffer solution can be calculated by using Handersson-Hesselbalch equation-

Q: Ka(HCN) = 6.2 x 10-10. Determine the pH of 0.82 M NaCN aqueous solution (3 significant figures).

A:

Q: I have some acetic acid that dissociates in water.  [CH3COOH]= .405 M [CH3C00]= .505 M Ka= 1.8 x…

A:

Q: calculate the pH of 20.00mL of a solution of acetic acid, HC2H3O2 0.105M with NaOH 0.105 M. For…

A:

Q: Classify each aqueous solution as acidic, basic, or neutral at 25 °C. Acidic Basic Neutral Answer…

A: Since you have posted questions with multiple subparts, we will solve the first three sub parts for…

Q: pproximate the final pH of a solution when 1.5 moles of a weak acid is added to water to a final…

A: Given : Moles of weak acid = 1.5 Volume = 1L Ka =  5.67x10^-8

Q: How many grams of NaOH (MW=40.0 g/mole) do you need to add to 50.0 ml of a 0.2 M weak acid HA…

A: Given data contains, Concentration of HA is 0.2 M. Volume is 50.0 mL. Ka is 4×10-6. The moles of HA…

Q: Calculate the concentration of an aqueous solution of NaOH that has a pH of 11.50 Group of answer…

A:

Q: Buffers remote

A: Given: Ionisation constant Ka = 1.8×10-5 Concentration of acetic acid = [HC2H3O2] = 0.1 M…

Q: find the  pH of a 0.00250 M solution of dimethylamine, (CH3)2NH? : Atoms First.  The ionization…

A: pH is used to determine the concentration of hydronium ion.

Q: Calculate the pH of a solution when 32.0 mL of 0.200 M formic acid (HCOOH, Ka = 1.77 x 10-4) is…

A:

Q: What is the pH (to two decimal places) of a 50.0 mL 0.15 M NH3 aqueous solution (at 25 °C) after…

A: Given data,Molarity of NH3=0.15MVolume of NH3=50mL=0.050LMolarity of HCl=0.20 MVolume of…

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: 0.100 moles of each substance is dissolved in 1.0 L of water. Decide if each is an acid or a base…

A: An acid is a substance that can furnish hydrogen ions in aqueous and the base increases the…

Q: A 50.0 mL solution of the weak acid HA (Ka = 1.00 × 10-6) has a pH of 4.000. What volume of water…

A: Given, Initial volume of HA  = 50.0 mL The initial pH value of HA at 50.0 mL = 4.000 The final pH…

Q: Determine the pH of a 0.625 M NH3 solution. The Kb of NH3 is 1.85 × 10-5.

A: Given,  The pH of a 0.625 M NH3 solution is: The Kb of NH3 is 1.85 × 10-5.

Q: Find the pH of a 0.4M aqueous hydrocyanic acid solution. For HCN, Ka=4.9 x 10^-10     4.85…

A:

Q: Ka for hypochlorous acid, HClO, is 3.0×10-8. Calculate the pH after 10.0 mL of 0.100 M NaOH have…

A: Given data : Volume of HClO = 40 mL Concentration of HClO = 0.100 M Volume of NaOH = 10 mL…

Q: Hydrofluoric acid (HF) has a Ka value of 7.2 x 10^-4. What is the pH to 2 decimal places when 13.75…

A: Given : Ka=7.2×10-4 Volume of KOH=13.75 ml Molarity of KOH=1.074 M Volume of HF=27.5 ml…

Q: Find the pH of each mixture of acids. a) 7.5×10−2 M in HNO3 and 0.175 M in HC7H5O2 b) 1.5×10−2 M in…

A: a) The hydrogen concentration of nitric acid and benzoic acid are calculated as,

Q: Ka for a 0.100 M hydrofluoric acid solution where whose pH is 2.23 is a. 3.5x10-4 b. 3.5x10-2 c.…

A: Hydrofluoric acid is a weak acid The equation representing dissociation of HF in water: HF + H2O →…

Q: Calculate the pH of a solution made by mixing 50.00 mL of 0.100 M NaCN with (a) 4.20 mL of 0.438 M…

A: You have posted 2 different  questions simultaneously, so I have to solve the first one that is 5…

Q: What is the pH of a 0.48 M triethylamine, (C2H5)3N, solution? Kb for triethylamine is 5.3 × 10–4

A: We have to find pH of a 0.48 M triethylamine, (C2H5)3N, solution

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.