How many grams of KNO2 (MM = 85.10 g/mol) must be added to 1.00 L of 0.132 M HNO2 to make a buffer solution with a pH of 3.63?

Q: How much 5.70 M NaOH must be added to 430.0 mL of a buffer that is 0.0180 M acetic acid and 0.0240 M…

A: Concentration of NaOH = 5.70 M Concentration of acetic acid = 0.0180 M Concentration of sodium…

Q: how many grams of NH4Cl must be added to 1 liter of 1.0 M NH4OH solution to prepare a buffer…

A:

Q: b) A buffer solution is prepared by adding 40.0 g of sodium acetate CH;COONA to 500 mL of a 0.200 M…

A: Given: Mass of CH3COONa =40.0g Molar mass of CH3COONa =82.03 g/mol Volume of solution =500ml=0.5 L…

Q: 4) Calculate the pH of a buffer that is 0.012 M C,H5COOH ( Ka= 6.3x10) and 0.033 M NaC6HsCOO.

A:

Q: How many microliters of 1.000 M NaOH solution mustbe added to 25.00 mL of a 0.1000 M solution of…

A: Find the moles of lactic acid.

Q: What is the pH of a buffer made from 0.580 mol of CH₃NH₂ (Kb = 4.4 × 10⁻⁴) and 0.180 mol of CH₃NH₃I?

A: Concentration of CH3NH2 = 0.580 Concentration of  CH₃NH₃I = 0.189 Kb = 4.4 × 10-4  pH = ?

Q: What mass of NH4Cl must be added to 0.750 L of a 0.100-M solution of NH3 to give a buffer solution…

A: Ammonia is a weak base and form a buffer solution with NH4Cl The pH of buffer is close to 9-10.…

Q: How many microliters of 1.000 M NaOH solution must be added to 25.00 mL of a 0.1000 M solution of…

A: Find the moles of lactic acid.

Q: What mass of NH4Cl must be added to 500 mL of a 0.150 M NH3 solution to make a buffer with pH =…

A: Step 1: Here, the ammonia NH3 solution is weak base and NH4Cl is its conjugate acid. The pKb value…

Q: How many moles of NH4Cl must be added to 3.0 L of aqueous 0.10 M NH3 to form a buffer whose pH is…

A: Adding ammonium chloride, NH4Cl, to an ammonia solution will effectively create a buffer solution…

Q: How many grams of solid ammonium bromide should be added to 2.00 L of a 0.274 M ammonia solution to…

A: Given data, pH of the buffer=8.530 This buffer is basic buffer. So,pOH=14-pH =14-8.530=5.47…

Q: What mass of Na2HPO4 must be added to 250. mL of 0.50 M H2PO4- to generate a buffer with a pH of…

A:

Q: How much 5.80 M NaOH must be added to 480.0 mL of a buffer that is 0.0185 Macetic acid and 0.0265 M…

A: given: pH = 5.75 For Acetic acid, pKa = 4.75  Let V mL of NaOH is needed. Millimoles of NaOH = 5.80…

Q: How much 5.50M NAOH must be added to 450.0 ml of a buffer that is 0.0180 M acetic acid and 0.0250 M…

A: Given CH3COOH(aq)+OH-(aq)→CH3COO-(aq)+H2O(l) We know that pKa= 4.75 pH=5.75 For the 0.0265M sodium…

Q: How many grams of solid ammonium bromide should be added to 2.00 L of a 0.205 M ammonia solution to…

A: Given data :

Q: How many grams of solid potassium hypobromite, KBrO must be added to 200.0 ml of 0.100M hypobromous…

A:

Q: How much 10.0 M HNO3 m

A:

Q: How many grams of solid sodium hypochlorite should be added to 1.50 L of a 0.185 M hypochlorous acid…

A: The given problem can be solved by using Henderson-Hasselbalch equation as; pH = pKa + log conjugate…

Q: A buffer is prepared by mixing 50.0 mL of 0.050 M sodiumbicarbonate and 10.7 mL of 0.10 M NaOH. (a)…

A: a.

Q: A buffer system is prepared that is 0.020 M in NH3 and 0.030 M in NH4 What is the pH after adding…

A: IMPORTANT POINTS: It is a basic buffer of aqueous solution of ammonia (NH4OH) and NH4+ ,Needless to…

Q: How much 5.80M NAOH must be added to 430.0 mL of a buffer that is 0.0215 M acetic acid and 0.0270M…

A:

Q: Consider a buffer made of carbonic acid H2C03 and its conjugate base NaHCO3 with a pH of 6.50. (Ka…

A: The Henderson- Hasselbalch equation provides a relationship between the pH of acid(in aqueous…

Q: What mass of sodium formate must be added to 400 mL of 1.00 M formic acid to produce a buffer…

A: We have to find mass of sodium formate must be added to 400 mL of 1.00 M formic acid to produce a…

Q: How many grams of solid ammonium bromide should be added to 1.50 L of a 0.106 M ammonia solution to…

A: From the relation, pOH is calculated as,

Q: How many grams of dry NH4Cl nned to be added to 2.50 L of a 0.200 M solution of ammonia, NH3, to…

A:

Q: 4. How many moles of NH4C1 must be added to 2.0 L of 0.10 M NH3 to form a buffer whose pH is 9.00?…

A: We have volume as 2L, 0.1 M NH3, pH is 9, Kb as 1.8*10-5. We have to calculate the moles of ammonia…

Q: How much 10.0 M HNO3 must be added to 1.00 L of a buffer that is 0.0100 M acetic acid and 0.100 M…

A: Given: pKa of acetic acid = 4.75 Concentration of acetic acid = 0.0100 M Concentration of sodium…

Q: A 500-ml sample of a 0.100 M formate buffer, pH 3.75, is treated with 5 mL of 1.00 M KOH. What is…

A: Buffer solutions The solution that resists any change in pH is called buffer. It is the mixture of…

Q: A buffer is prepared by adding 45 ml of 0.15 NaF to 35 ml of 0.1 M HF. What is the pH of the final…

A: Interpretation -  To determine the pH of the final solution when a buffer is prepared by adding 45…

Q: A buffer is prepared by adding 10.0 g of ammonium chloride(NH4Cl) to 250 mL of 1.00 M NH3 solution.…

A:

Q: How much 6.01 M NAOH must be added to 590.0 mL of a buffer that is 0.0210 Macetic acid and 0.0230 M…

A:

Q: What mass of sodium acetate (NaOAc, 82.03 g/mol) would be needed to prepare 1L of the pH 5.000 0.100…

A:

Q: 3) A student made a buffer using 0.750 moles of HCN and 0.250 moles of NaCN dissolved into 2.00L of…

A: Given that : Number of moles of acid (HCN) = 0.750 moles Number of moles of base (NaCN) = 0.250…

Q: 6.75 grams of sodium benzoate, NaC7H5O2, is added to 1.00 L of a 0.25 M benzoic acid solution…

A: Given-> Weight of sodium benzoate = 6.75 gm Volume of benzoic acid = 1.00 L Molarity of benzoic…

Q: What is the pH of a buffer solution containing 0.4M NaOCl and 0.2 mol of HOCl with Kb of OCl is…

A:

Q: A buffer is made by adding solid sodium citrate (Na3C6H5O7) to a solution of 1.20 M-Na2HC6H5O7. The…

A: Na2HC6H5O7 is a weak acid with pKa value of approximately 6.39 Na3C6H5O7 is the conjugate base of…

Q: What is the pH of a buffer made from 0.580 mol of CH₃NH₂ (Kb = 4.4 × 10⁻⁴) and 0.120 mol of CH₃NH₃I?

A: In this question, we want to determine the Calculate the pH of the buffer solution.  You can see…

Q: What mass of NaCH3COO should be added to 1.00 L of 0.100 M CH3COOH to produce a buffer solution with…

A: pKa(CH3COOH) = 4.74  Molar mass of salt(S) = 82.03 g/mol Assume, moles of NaCH3COO(S) = n moles…

Q: How many grams of solid ammonium bromide should be added to 1.50 L of a 0.162 M ammonia solution to…

A:

Q: How much 6.01 M NaOH must be added to 470.0 mL of a buffer that is 0.0185 M cetic acid and 0.0230 M…

A: The given data: The molarity of NaOH =6.01 M. The volume of the buffer solution= 470 mL. The…

Q: What volume of 0.200 M HCl must be added to 250.0 mL of 0.300 M sodium mandelate to produce a buffer…

A: An acidic substance is the substance that can give H+ ions. They are corrosive and sour in nature.…

Q: How many moles of CH₃NH₃Cl  need to be added to 200.0 mL of a 0.500 M solution of CH₃NH₂ (Kb for…

A: Given, Volume of solution (v) = 200 mL = 0.2 L Molarity of Base (M) = 0.500 M Kb of base = 4.4×10⁻⁴…

Q: How much 5.50 M NaOH must be added to 580.0 mL of a buffer that is 0.0200 M acetic acid and 0.0275 M…

A:

Q: 3. A buffer solution contains 0.125 moles of ammonium chloride added to 500.0 ml of 0.500 M solution…

A:

Q: Calculate the pH of a 1.000 L buffer solution that: a. initially consists of 0.0400 moles of NH3 and…

A: Given     1 L  of buffer solution consists of 0.0400 moles of  NH3and 0.0250 moles of  NH4+…

Q: How many moles of CH;NH;CI need to be added to 200.0 mL of a 0.500 M solution of CH3NH2 (Kb for…

A: The solution is a buffer solution of weak base CH3NH2 and its conjugate acid CH3NH3Cl.

Q: How many grams of NH4CI would have to be added to 250.0 mL of a 0.420 M NH3 solution to prepare a…

A: The minimum concentration of NH4Cl that must be present in the solution to have a pH of 10 is;…

Q: How many grams of solld ammonium chloride should be added to 0.500 L of a 5.15x10-2 M ammonla…

A: Given,  Molarity of  ammonia = 5.15 × 10-2 M.  Volume = 0.500L. The pH of the buffer is 8.730  The…

Q: How many grams of solid potassium hypobromite, KBrO must be added to 500.0 ml of 0.500M hypobromous…

A:

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.