n analytical chemist is titrating 94.2 mL of a 0.4600M solution of dimethylamine ((CH;),NH) with a 0.2300M solution of HNO,. The p K, of dimethylamine s 3.27. Calculate the pH of the base solution after the chemist has added 121.9 mL of the HNO, solution to it. Vote for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places.

Q: Calculate the pH of 50.00 ml distilled water after the addition of 4.00 ml 0.10 M HCl. 2. Calculate…

A: Given the volume of distilled water = 50.00 mL Volume of 0.10 M HCl added = 4.00 mL * (1L/1000 mL) =…

Q: A chemist titrates 110.0 mL of a 0.3936M dimethylamine ((CH3), NH) solution with 0.7244M HNO,…

A:

Q: Calculate pH for a strong acid/strong base titration. Determine the pH during the titration of 23.2…

A:

Q: A buffer system is prepared by combining 0.406 moles of ammonium chloride (NH4CI) and 0.525 moles of…

A: Moles of base (NH3 ) = 0.525 mol  Moles of conjugate acid (NH4+ ) = 0.406 mol Moles of nitric acid…

Q: pH for a weak base'strong acid titration. Determine the pH during the titration of 37.6 ml. of 0.319…

A:

Q: A chemist titrates 120.0 mL of a 0.2898M carbonic acid (H₂CO,) solution with 0.8540M KOH solution at…

A: pH value at equivalence point can be calculated by considering the equilibrium reaction of HCO3-

Q: An analytical chemist is titrating 111.3 mL of a 0.2800 M solution of ammonia (NH,) with a 0.3500 M…

A: The chemical equation may be written as: Given data is: solution of ammonia = 111.3 mL Molarity of…

Q: An analytical chemist is titrating 107.8 ml. of a 0.1900M solution of dimethylamine ((CH,) NH) with…

A:

Q: A buffer solution could be made by mixing equal amounts of citric acid and a solution containing.…

A: Given a citric acid buffer solution. Fill the correct option.

Q: 8. A 100. mL sample of 0.10 MHCI is mixed with 50. mL of 0.12 M NH.. What is the resulting pH? (K,…

A: Reaction taking place between NH3 and HCl is shown below, NH3+HCl  → NH4Cl Here, one mole of salt…

Q: In the laboratory, a general chemistry student measured the pH of a 0.430 M aqueous solution of…

A: Hypochlorous acid is a weak acid. So we can use the equation for the pH for weak acid to solve this…

Q: What will the pH be when 50 mL 0.01 M acid with pKa of 1.0*10^(-0.5) is mixed with 1. 25 mL 0.01M…

A: No. of moles = Molarity*Volume Moles of acid= 0.01 * (50 mL / 1000 mL/L)= 0.0005 molesCalculation of…

Q: An analytical chemist is titrating 159.6 ml. of a 0.7000 M solution of diethylamine ((GH), NH) with…

A:

Q: A chemist titrates 20.0 mL of 0.20 M HBrO (see Appendix) with 0.10 M NaOH. What is the pH: c) at…

A:

Q: An analytical chemist is titrating 207.7 mL of a 0.2900M solution of acetic acid (HCH,CO,) with a…

A: We will calculate pH

Q: Determine the pH during the titration of 28.1 ml of 0.170 M hydroiodic acid by 0.136 M sodium…

A: Given,  Volume HI = 28.1 mL  Molarity of HI = 0.170 M  Molarity of NaOH = 0.136 M  (1). What is the…

Q: An analytical chemist Is titrating 100.6 mL of a 0.7200M solution of ammonla (NH,) with a 0.4000M…

A:

Q: An analytical chemist is titrating 222.0 mL of a 0.6100 M solution of hydrazoic acid (HN,) with a…

A: Given: Concentration of HN3 (M1) = 0.6100 M Volume of HN3 (V1) = 222.0 mL Concentration of NaOH (M2)…

Q: The buffer capacity of a solution is 0.02 .How much(ml) of 1.0 M solution of sodium hydroxide NaOH)…

A: Buffer solution :- A solution which resist the change in its pH value by the addition of small…

Q: An analytical chemist is titrating 94.4 mL of a 0.5900M solution of ammonia (NH, with a 0.1400M…

A: Buffer solution: A buffer solutions is an aqueous solution consisting of a mixture of a weak base…

Q: The p?a of hypochlorous acid is 7.530 . A 58.0 mL solution of 0.130 M sodium hypochlorite ( NaOCl )…

A: Answer: Buffer solution is a type of solution that resists the change in its pH on adding small…

Q: What is the pH of a buffer solution that is 0.493 M in hydrofluoric acid and is 0.483 M is potassium…

A: Concentration of acid (HF) = 0.493 M  Concentration of conjugate base(KF) = 0.483 M  Ka of HF = 6.4…

Q: Out of the following, which is incorrect? been pleed (2 lortrymond (b a) A buffer solution is one…

A: A buffer solution is a mixture of two solutions - a weak acid and its conjugate base. It has a…

Q: An analytical chemist is titrating 15.3 ml of a 0.4200M solution of hydrazoic acid (HN,) with a…

A:

Q: What is the pH of a buffer solution that is 0.416 M in ammonia and 0.406 M in ammonium chloride…

A:

Q: The theoretical pK, of a weak acid is 3.54. Calculate the pK, experimental error of a solution…

A: weak acid and its salt of conjugate base with strong base forms acidic  buffer whose pH is…

Q: 16.35 A 25.0-mL solution of 0.100 M CH;COOH is ti- trated with a 0.200 M KOH solution. Calculate the…

A: a) 0.0 mL Ka of CH3COOH = 1.8×10-5 Now, the hydrogen ion concentration is, [H+] = √Ka × 0.100 M [H+]…

Q: A solution is prepared that is initially 0.17 M in trimethylamine ((CH,),N), a weak base, and 0.20 M…

A:

Q: An analytical chemist is titrating 221.9 mL of a 0.8100M solution of diethylamine ((C,H3),NH) with a…

A: Given that, 221.9 mL of a 0.8100 M solution of diethylamine [(C2H5)2NH] is titrating with a 0.7200 M…

Q: with a 0.7900 M solution of HNO,, The p K, of An analytical chemist is titrating 102.2 mL of a…

A:

Q: A chemist titrates 150.0 mL of a 0.0676M dimethylamine (CH,) NH) solution with 0.4402M HBr solution…

A: Interpretation - To calculate the pH at equivalence point.     Given  molarity of dimethyl amine =…

Q: of a 0.8100M solution of dimethylamine (CH),NH) An analytical chemist is titrating 106.9 mL NH with…

A: The question is based on the concept of titrations.   we are titrating  a weak dimethylamine base…

Q: An analytical chemist is titrating 204.9 ml. of a 0.2200M solution of cyanic acid (HCNO) with a…

A:

Q: An analytical chemist is titrating 109.3 ml. of a 0.8700M solution of butanoic acid (HC,H,CO,) with…

A: A buffer is a solution which resist any change in pH on adding a small amount of acid or base . It…

Q: An analytical chemist is titrating 187,7 ml. of a 0.4400M solution of isopropylamine ((CH,), CHNH,)…

A:

Q: When 35 mL of 0.20 M acetic acid and 35 mL of 0.10 M calcium hydroxide are combined, the pH of the…

A: Given : Concentration of acetic acid i.e CH3COOH = 0.20 M Concentration of calcium hydroxide i.e…

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.