a solution is made from 0.23 M CH3NH2 (a weak base) and 0.24 M CH3NH3Cl. what is the pH of the solution if the Kb for CH3NH2 is 4.4x10^-4?

Q: A solution is prepared that is initially 0.27M in hypochlorous acid (HCIO) and 0.34M in sodium…

A: The concentration of the hypochlorous acid The concentration of the sodium hypochlorite We have to…

Q: 3. (a) A 20.0 mL sample of 0.200 M cyanic acid (HOCN, K₁=3.3 x 104) is titrated with 0.400 M NaOH.…

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Q: A solution is prepared that is initially 0.27M in methylamine (CH3NH₂), a weak base, and 0.21M in…

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

Q: Calculate the pH of the resulting solution if 31.0 mL of 0.310 M HCl(aq) is added to 41.0 mL of…

A: Answer: When acid and base solution are mixed then water and salt forms, this reaction is called as…

Q: You are studying a clear solution and you added the pH indicator methyl violet. The colour range of…

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Q: You add 100.0 mL of 0.50 M NaOH to 50.0 mL of 1.00 M NH4CI. What is the pH of the resulting…

A: Ammonia(NH3) is a weak base whose base dissociation constant is given as Kb=1.8×10-5 while ammonium…

Q: A chemistry graduate student is given 125.mL of a 1.00M methylamine CH3NH2 solution. Methylamine is…

A: pH of buffer solutions can be calculated using Henderson-Hasselbalch equation. pOH of basic buffer…

Q: An analytical chemist is titrating 136.3 mL of a 0.1300M solution of ammonia (NH3) with a 0.1800M…

A: Here we required to find the pH of the solution.

Q: A 100. mL sample of 0.10 M HCl is mixed with 50. mL of 0.14 M NH3. What is the resulting pH? (Kb for…

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Q: Given that Ka’s for hydrofluoric acid (HF) and boric acid (H3BO3) are 6.3 × 10^–4 and 5.4 × 10^–10,…

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Q: If a buffer solution is made from 300.0 mL of 2.2 M pyridine salt mixed with 350.0 mL of 2.0 M…

A: Buffer solution pH is determined using Henderson–Hasselbalch equation. Which relates salt…

Q: 4. Formic acid, HFor, has a K, value equal to about 1.8 × 10¬4. A student is asked to prepare a…

A: A buffer solution is formed by the mixture of acid and its conjugate base in such a way so that it…

Q: b An analytical chemist is titrating 136.2 mL of a 0.7100M solution of methylamine (CH3NH2) with a…

A: Given: VCH3​NH2​​=136.2mL;[CH3​NH2​]=0.7100M;VHNO3​​=97.5mL;[H+]=0.4900MpKb​=3.36;pH=???Step 1:…

Q: When a small amount of 12 M HNO3(aq) is added to a buffer solution made by mixing CH3NH2(aq) and…

A: Buffer solution is made by mixing weak acid and its salt with strong base (or) by mixing weak base…

Q: Calculate the pH of a solution that is 0.0120 M in HCl and 0.0550 M in picric acid. pH = Submit b…

A: Hello. Since your question has multiple sub-parts, we will solve first three sub-parts for you. If…

Q: a) Calculate the pH of the solution formed when 100 cm³ of 0.100 mol dm³ H₂SO, is added to 50 cm³ of…

A: Pls repost your question ( 5) .

Q: A solution is 0.40 M HF and 0.80 M KF. Which of the following actions will result in pH - pK, for…

A: solution which resists it pH by adding small amount strong acid (or) strong base is called buffer…

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Q: Given that Ka’s for hydrofluoric acid (HF) and boric acid (H3BO3) are 6.3 × 10^–4and 5.4 × 10^–10,…

A: a) Given: Volume of HF=50 mL Concentration of HF= 0.2 M Concentration of NaH2BO3= 0.5 M Volume of…

Q: In a titration experiment of a 25.00 mL of 0.100M CH3CO2H with 0.100 M NaOH, 12.50 mL of NaOH were…

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

Q: A 2.00 L solution contains 0.545 M NH3 and 0.641 M NH4A.  (The Kb of NH3 is 1.86⋅10−51.86⋅10-5).…

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Q: If a buffer solution is made from 300.0 mL of 1.6 M aniline salt mixed with 250.0 mL of 2.0 M…

A: Given: Concentration of aniline salt = 1.6 M Concentration of aniline = 2.0 M Volume of aniline salt…

Q: A solution is prepared that is initially 0.45M in pyridine (C₁H₁N), a weak base, and 0.50M in…

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Q: An analytical chemist is titrating 64.8mL of a 0.3000M solution of ammonia NH3 with a 0.7300M…

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Q: A solution is prepared that is initially 0.13M in acetic acid (HCH₂CO₂) and 0.24M in potassium…

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Q: A 2.00 L solution contains 0.678 M NH3 and 0.670 M NH A. (The Kb of NH3 is 1.86 10-5). What is the…

A: #1: NH3 is a weak base and NH4A or NH4+ is a conjugate acid or NH3. Hence the solution acts as a…

Q: NOTE: The following 4 questions involve the titration of a 50.00 mL sample of 0.200 M chlorous acid,…

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Q: A buffer solution is 0.337 M in H2CO3 and 0.239 M in KHCO3 . If Ka1 for H2CO3 is 4.2x10^-7 , what…

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Q: A solution is prepared that is initially 0.27 M in hypochlorous acid (HCIO) and 0.34M in sodium…

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Q: A Titration of 10.0 mL of 0.15 M NaOH is added 0.35 M HNO3. What is the volume of HNO3 to reach…

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Q: A chemist starts her experiments with 25.00 mL of 0.125 mol L-1 NaCN solution. The pKa of HCN =…

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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.