. Which of the following combinations would act as buffered solutions?a. HCl and NaClb. CH3COOH and KCH3COOc. H2S and NaHSd. H2S and Na2S

Q: What mass of HI must be present in 0.250 L of solution to obtain a solution with each pH value?a. pH…

A: Given, volume of solution = 0.250 L HI is a strong electrolyte and it ionizes in solution as,…

Q: Calculate the pH of a solution made by adding 15.0 mL of 0.200 M HCl to 150 mL of 0.100 M NH3…

A: The relation to determine the pH of buffer solution is given by Henderson-Hasselbalch. The relation…

Q: A concentrated HCl solution contains 36.0% HCl (density of 1.18 g/mL). How many liters are required…

A: pH: The acidity of the solution is given in the term of pH, it is given by negative logarithm of…

Q: A chemist makes four successive 1:10 dilutions of 1.0X10⁻⁵ M HCl. Calculate the pH of the original…

A: The pH of a solution is the negative of logarithm of the concentration of hydrogen ions in the…

Q: A certain weak base has a ?b of .8.40×10−7. What concentration of this base will produce a pH of…

A: Assuming the weak base is monoprotic which can be written as BOH. Hence the dissociation reaction of…

Q: Which of the following combinations would act as buffered solutions? a. HCl and NaCl b. CH3COOH and…

A: Buffer solution: A buffer is a solution that can resist pH change upon the addition of an acidic or…

Q: You are given three solutions: HCl (Solution A); NaOH (Solution B); pH = 8.76 solution (Solution S).…

A: Given: Three solutions: HCl (Solution A); NaOH (Solution B); pH = 8.76 solution (Solution S) As the…

Q: Consider the following ions: Cl-, HS-, NO2-, F-, and HS04-. (a) Which of these ions in water gives…

A: Given ions  Cl- HS- NO2- F- HSO4-

Q: How will the amount of the unionized acid HA be affected (increased, decreased, unaffected can’t…

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

Q: What mass of HCI should be used to make 175.0 ml of a solution with a pH of 2.80? The molar mass of…

A: Provided volume (V)=175ml Or, Provided volume (V)= 0.175litre Provided molar mass of HCl=36.46g/mol…

Q: which assumption can't be applied in the calculation of the pH of this solution? (a) that the…

A: pH is the measure of the concentration of the H+ ions in the solution. It can be acidic, basic, and…

Q: Calcium carbonate is a common ingredient in antacids that reduces the discomfort associated with…

A: Given data Mass of CaCO3 = 39 mg pH of HCl solution = 1.60  Neutralization of CaCO3 using acid HCl…

Q: 25.0 g sample of CH3COONa is completely dissolved in 500.0 mL of water and CH3COOH has an acid…

A: Given: Mass of CH3COONa = 25.0 g. And volume of solution = 500.0 mL = 0.500 L…

Q: The pH of an aqueous solution at 25°C was found to be 5.80. The pOH of this solution is .????? The…

A:

Q: A solution of formic acid (HCOOH) has a pH of 2.36. How many grams of formic acid are there in…

A: Given that pH of formic acid is 2.36 Molecular weight of HCOOH = 46 grams.

Q: III. A solution is made by adding 10-3 M HOCI and 10-3 M NaPr to water. Then, NaOH is added until…

A:

Q: Part A If 15.0 mL of glacial acetic acid (pure HC2H3O2; K₂ = 1.8 × 10−5) is diluted to 1.70 L with…

A:

Q: If 5.00 mL of 0.500 M NaOH are added to 10.00 mL of 0.300 M HCl, what is the final pH?

A: pH is used to measure the concentration of hydronium ion.  The expression for the calculation of pH…

Q: A certain weak base has a ?bKb of 8.80×10−7.8.80×10−7. What concentration of this base will produce…

A: 0.057 M

Q: Calculate the pH of a solution formed by mixing 65 mL of a solution that is 0.34 M in NaHCO3 with 75…

A:

Q: For each strong acid solution, determine [H3O+], [OH-], and pH.a. 0.25 M HClb. 0.015 M HNO3c. a…

A: Hello. Since the question contains more than three sub-parts, the first three sub-parts shall only…

Q: Diluted sulfuric acid has a density of 1.3 g / ml and contains 39% by mass of H2SO4. a) What is the…

A:

Q: Some calcifies can use bicarbonate (HICO3-) to make the shells. How will they be affected by the…

A:

Q: Consider a HCI solution with a pH of 4.70. a) Calculate the concentration of HCl. b) Identify the…

A: pH is he negative logarithm of hydrogen ions. pH values can range from 0 to 14. pH is used to know…

Q: Which of the following combinations would act as buffered solutions?

A: ANSWER

Q: Calculate the pH of a 1L aqueous solution that is0.14 M in HF and 0.19 M in NaF after 0.013 mol of…

A: The solution which can resist the change in the pH of solution upon addition of acid or base is…

Q: 3 60.0 ml of NaOH, the pH of the resulting solution is greater than 7. g 20.0 mL of NaOH, the pH of…

A: Mmol of formic acid = M × V     = 0.60 × 40 = 24 mmol After adding 60 mL of NaOH,  Mmol of NaOH =…

Q: What is the concentration of hydroxide ion in a 0.160 M  aqueous solution of hydroxylamine, ? What…

A: Given: The concentration of the aqueous solution of hydroxylamine (NH2OH) is 0.160 M The Kb value is…

Q: A 30.0 mL aliquot of a solution is 0.25 M HCl . If 0.1 M NaOH is to be added to this solution,…

A:

Q: Each box represents an aqueous solution of a weak acid, HX, and its conjugate base, X¯. Water…

A:

Q: 1.0 mL of 2M HCl added to 1.00 L pure water Calculate moles of 2 M HCl, then concentration of…

A: Given : Concentration of stock solution of HCl = 2 M Volume of stock solution taken = 1.0 mL = 0.001…

Q: a solution of NaOH is 0.2 M and has a density of 1.2 g / mol. a) What is the pH of this solution? b)…

A: Given : (a) [NaOH] = [OH-] = 0.2 M  pOH = -log[OH-] = -log 0.2 = 0.7  pH = 14 - 0.7 = 13.3  (b)  By…

Q: 7.30×10−7. What concentration of this base will produce a pH of 10.14?

A:

Q: A general chemistry student mixes together a solution of HF with a solution of NaF. If the resulting…

A: Acidic buffer solution :- A mixture of weak acid and its salt with strong base is called acidic…

Q: Calculate the molar concentration of the base.

A: Molarity is used to express the concentration of a solution. Molarity is the number of moles of…

Q: You add 15.00 mL of 0.700 M NaOH to 50.00 mL of pure water, and to this mixture you then add 5.00 mL…

A: Given: concentration of NaOH = 0.70 M volume of NaOH = 15.0 mL volume of water = 50.0 mL Volume of…

Q: A certain weak base has a ?b of 8.40×10−7. What concentration of this base will produce a pH of…

A: Weak base dissociated less in solution

Q: Calculate the pH of a solution made by diluting 11 mL of a 3 M solution of HCI to a final volume of…

A: Initial Molarity of HCl solution = M1 = 3 MInitial Volume of HCl solution = V1 = 11 mL= 0.011 LFinal…

Q: Fill in the blanks. When an acid is added to pure water the increases and the decreases. O A) H30*…

A: An acid is a substance which increases concentration of H3O+ in solution. Note :- acid has pH<7…

Q: A solution of housechold bleach contains 5.25% sodium hypochlorite, NaOCI, by mass. Assuming that…

A: For a salt formed by weak acid and strong base, PH is given by  PH = 7 + 1/2 PKa + 1/2 log C  Where…

Q: Calculate the pH of solution of 1 ml of 6.0M HCI added to 32.2 mL Of pure Water with a recorded pH…

A: Given: 1 mL of 6 M HCl added to 32.2 mL of pure water with pH = 8.52  pH = - log [H+] 8.52 = - log…

Q: A certain weak base has a ?b of 7.90×10−7. What concentration of this base will produce a pH of…

A: As per the given information  certain weak base has a kb is 7.90×10-7. pH=10.03 The chemical…

Q: Calculate the pH of each of the following strong acid solutions:(a) 0.0167 M HNO3, (b) 0.225 g of…

A: To calculate pH of each of strong acid solutions: (a). 0.0167 M HNO3

Q: 1.00 L of hydrochloric acid is prepared and has a final pH of 1.045. What mass of HCl) is dissolved?…

A:

Q: How many mL of 0.500 M NaOH should be added to 10.0 g tris HCI to give a pH of 7.60 in a final…

A: Here is your answer...........

Q: The PH of a solution of HCL in water is found to be 2.50.what volume of water would you add to 1.00L…

A: The given value of pH = 2.50 is present in 1 L of water . As we know as the pH value increases the…

Q: ou are given the following ; KBr, NH3, NaOCl, NH4Cl they are all 1 M aqueous solutions some other…

A: The given four compounds are KBr, NH3, NaOCl, NH4Cl. The concentration of each compound in the…

Q: op your selection from the following list to complete the answer: NaF HI HF HCI, KCI, H,NNH3…

A: Acidic solution has pH less than 7 Basic solution has pH greater than 7 and  neutral solution has pH…

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.