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: When 0.412 g of a weak base with Kb = 3.10 ×10-5 the base is dissolved in 1.00 L of solution, it has…

A: Assuming the molar mass is M  Hence moles of base = mass / molar mass = 0.412 / M And concentration…

Q: uppose a solution of NaOH was titrated and found to have a molarity of 0.250 M. This solution is now…

A:

Q: A 0.400 M solution of a weak base has a pH of 9.65. What is the base hydrolysis constant, K₁, for…

A:

Q: A buffer is prepared by using 0.20 mole of C6H5COOH and 0.40 mole of C6H5COO- in 1.00 liter of…

A: The objective of this question is to determine whether the buffering capacity of a solution,…

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: You mix 15.0 mL of 0.200 M NH4Cl with 15.0 mL of 0.400 M NH3. What is the pH of the resulting…

A: Given: Concentration of NH4Cl = 0.200 M Volume of NH4Cl solution = 15.0 mL = 0.015 L…

Q: When 0.020 mol of NaOH is added to 400. mL 0.250 M NH3/ 0.150 M NH4Cl buffer solution, the pH of the…

A: The question is based on the concept of buffer solution.   A buffer is a solution which resist any…

Q: LIOH+HNO3 → H₂O + Li NO3 200.0 mL of a 0.100 M solution of LiOH is mixed with 250.0 mL of a 0.100 M…

A: The question is based on the titrations. we are titrating a strong acid nitric acid with a strong…

Q: A buffer solution is made that is 0.488 M in H2CO3 and 0.488 M in KHCO3. If Ka1 for H2CO3 is…

A: Given: H2CO3 = 0.488 M KHCO3 = 0.488 M Ka = 4.20×10-7 pka =-log ka         = -log (4.20×10-7)…

Q: A solution is prepared that is initially 0.27 M in benzoic acid (HC,H,CO,) and 0.11 M in sodium…

A: The magnitude of an ionization reaction's equilibrium constant can be used to calculate the relative…

Q: Consider a 1.0-L solution that is 0.280 M C5H5N and 0.46 M C5H5NHCl at 25 °C. What is the pH of this…

A: The question is based on the concept of PH calculation. using henderson equation, we calculate…

Q: A buffer solution is 0.478 M in H3PO4  and 0.362 M in NaH2PO4 . If Ka1 for H3PO4  is 7.5 x 10^-3 ,…

A: According to the Henderson Hasselbalch equation is given by, Ph = Pka + log ([salt] / [acid] ) The…

Q: How many milliliters of 0.0200 M Ca(OH)₂are required to neutralize 79.7 mL of 0.0300 M HCl?

A: B

Q: Phosphoric acid is a triprotic acid (Kal To find the pH of a buffer composed of H₂PO¯ (aq) and…

A: The Ka values for the phosphoric acid areThe phosphoric acid has the following ionizations  H3PO4 ⇌…

Q: ) How many moles of BHCl (acidic salt) would need to be added to 452 mL of 1.66 M B (a weak base) to…

A: The question is based on the concept of buffer solution.   A buffer is a solution which resist any…

Q: 3/3.5 6377 100 9. If a 50.0-mL sample of 0.250 M NaCN is titrated by 20.0-mL of 0.250 M HCI (strong…

A: To determine the pH of the solution resulting from the titration, we need to consider the reaction…

Q: A solution (total volume = 1L) of 0.4 M NH3 contains 12.78 g of NHẠCI (MW = 53.491 g/mol). Kb = 1.8…

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Q: Calculate the pH of a buffer solution made by mixing 185.8 mL of a 1.56 M propanoic acid…

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Q: You need to prepare a pH = 9.20 buffer solution containing NH3 and NH4Cl. If you start with 0.63 M…

A: Buffer Question and finding the concentration of Salt to make a buffer of pH = 9.2

Q: a) Find the pH of a 500 mL aqueous buffer solution prepared with 3.81 g of H3BO3 and 4.55 gof…

A:

Q: A buffered solution containing disolved aniline, C6H5NH2, and aniline hydrochloride, C6H3NH3Cl, has…

A: A. Given that : pH of the buffer solution = 5.71 Concentration of base (C6H5NH2) = 0.290 M The pKb…

Q: E. Bob has a bottle of Chloric Acid that had a molarity of 0.5 and there was 400 ml of it in the…

A: Solution :  pH       pH is a quantitative measure for the acidity or basicity of the solution. This…

Q: If a buffer solution is 0.230 M in a weak base (Kb = 4.7 × 10 − 5 ) and 0.540 M in its conjugate…

A: The solution which resist any change in their PH is called buffer solution. Given , concentration of…

Q: Consider the titration of 145.0 mL of 0.100 M HCl by 0.250 M NaOH. Part 1 Calculate the pH after…

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Q: A buffer solution contains dissolved C₆H₅NH₂ and C₆H₅NH₃Cl. The initial concentration of C₆H₅NH₂ is…

A: A solution which is a mixture of weak acid and its conjugate base is known as buffer. For…

Q: A chemistry graduate student is given 100. mL of a 1.40M methylamine (CH3NH2) solution. Methylamine…

A: pKb  = - log Kb            =  - log (4.4  * 10-4 )          = 3.36pKa = 14-pKb       = 14- 3.36…

Q: A 1.0 liter solution contains 0.25 M hydrogen fluoride (HF) and 0.38 M sodium fluoride (NaF). What…

A: Buffer solution: The solution that resists the change in pH is known as a buffer solution. The…

Q: What is the pH of a solution of 0.15 M formic acid (HCOOH)? (Ka = 1.8 x 10-4) A 5.57 B 2.37 C) 2.28…

A:

Q: what is the pH?

A: Given :-  Concentration of weak base = 0.120 M  Concentration of conjugate acid = 0.590 M  Kb = 5.9…

Q: A chemistry graduate student is given 100. mL of a 0.40M chlorous acid (HCIO₂) solution. Chlorous…

A:

Q: Use the References to access important values if needed for this question. A buffer solution is made…

A: Given Data :  Concentration of H2S = 0.346M Concentration of NaHS = 0.346M Ka1 = 1.00 x 10-7  We…

Q: 6. Calculate the pH of the solution that results when0.093 g of Mg(OH)2 is mixed with 75.0 mL of…

A:

Q: Silver sulfide is formed by the interaction of silver and hydrogen sulfide based on the equation…

A: Given :-  [H2S] = 6.32×1000/300 = 21.07M  [Ag2S] = 30M  PKa = -log(Ka) = -log(9.6×10-8) = 8- 0.98 =…

Q: If a buffer solution is 0.100 M in a weak base (Kb = 4.7 × 10 − 5 ) and 0.440 M in its conjugate…

A: To find the pOH of the buffer solution, we need to use the Henderson-Hasselbalch equation, which is…

Q: If a buffer solution is 0.250 M in a weak acid (?a=2.3×10^−5) and 0.440 M in its conjugate base,…

A:

Q: access Important values if needed for this question. A buffer solution is made that is 0.497 M in…

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

Q: Consider the reaction of 75.0 mL of 0.350 M C₅H₅N (Kb = 1.7 x 10⁻⁹) with 100.0 mL of 0.425 M HCl.…

A: Given: Volume of C₅H₅N = 75.0 mL Concentration of C₅H₅N = 0.350 M Volume of HCl = 100.0 mL…

Q: Formic acid, HFor, has a Ka value of 1.8 x 10^-4. You need to prepare a buffer having a pH of 3.25…

A:

Q: A solution contains 0.363 M HA (Ka = %3D 6.74-10-46.74-10-4) and 0.677 M NaA. What is the pH of this…

A: A solution contains 0.363 M HA and 0.677 M NaA.Ka of HA is 6.74 × 10-4We have to calculate the pH…

Q: A buffer solution is 0.405 M in H2CO3 and 0.397 M in KHCO3. If Kal for H2CO3 is 4.2 × 107, what is…

A: The objective of the question is to calculate the .

Q: 2. If you make a solution by mixing 25.mL of 0.50 M acetic acid (CH3COOH) and 25 mL of 0.30 M sodium…

A: Given,  [CH3COOH] = 0.50 M  Volume of CH3COOH = 25 mL  [CH3COONa] = 0.30 M  Volume of CH3COONa = 25…

Q: A solution is prepared that is initially 0.23 M in pyridine (C,H,N), a weak base, and 0.47M in…

A:

Q: 70 ml of an aqueous solution of 0.085 M acetic acid. It has a Ka=2.25x10^-4. Calculate the ph of the…

A: In the presence of strong acid the dissociation of weak acid is suppressed due to common ion effect…

Q: A student peforms a titration, titrating 25.00 mL of a weak monoprotic acid, HA, with a 1.14 M…

A: Given: Concentration of NaOH = 1.14 M Volume of HA solution used = 25.0 mL = 0.025 L…

Q: pH of the mixture of 0.020 M NH3 and 0.15 M NH4Cl (Kb NH3 =1.8*10^-5

A: Recall the Henderson-Hasselbalch equation to calculate pH of buffer solution       pOH=pKb +…

Q: 20. mL of 0.250 M NH3 is titrated with 0.500 M of HCl solution, what is the pH of the resulting…

A: Given data,Molarity of NH3=0.250MVolume of NH3=20mLMolarity of HCl=0.50MKb=1.8×10-5

Q: 4) What is the pH of a buffer solution, prepared by mixing of 75 mL 0.1 M CH3COOH solution and 150…

A: In this question we have to tell the PH of the buffer 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.