When 25.0 mL of 0.400 M hydrobromic acid and 25.0 mL of 0.400 M potassium nitrite are combined, the pH of the resulting solution will be : A. Less than 7 B. Equal to 7 C. Greater than 7

Q: Explain why the pH does not change significantly when a small amount of an acid or a base is added…

A: Option D is correct

Q: ph of 5% white vinegar is 2.22 Caculate the molarity. (5.00g acetic acid/ 100.00g solution) *asume…

A: Molarity is defined as “the mole of the solute per unit volume of the solution”. It is represented…

Q: Calculate the pH of the following solutions. a) 0.400 M HCl solution  b) Solution containing 0.727…

A:

Q: 14. Which indicator in yellow in a solution with a pH of 987 A methyl ornge R. hromthymol Mue C…

A: We have to tell which option is correct

Q: what volume of 0.10 M sodium acetate must be added to 20.0 ml of 0.20 M acetic acid to produce a…

A: The Henderson Hasselbalch equation for acidic buffer is given as :

Q: 1) A 50.0 mL solution of 0.107 M KOH is titrated with 0.214 M HCI. Calculate the pH of the solution…

A: Given,Molarity of KOH = 0.107 Mvolume of KOH = 50.0 mLMolarity of HCl = 0.214 Mvolumes of HCl are:a.…

Q: A student titrates 25 mL of an acid with 0.20M NaOH. if it takes 40.0 mL of NaOH to reach of pH of…

A:

Q: What is the pH of a solution

A:

Q: 3. a. Find the pH of a solution that is 0.25 M NH, and 0.10 M NH.CI given that the K. for NH" is…

A:

Q: What is the pH, when 20 ml 0.01 M NaOH is added to 100 ml 0.02 M HCI? Select one: a. 0.015 b. 1.82…

A: An acid base titration is an experimental technique which is used to acquire information about a…

Q: When 25.0 mL of 0.300 M hydrobromic acid and 25.0 mL of 0.300 M ammonia are combined, the pH of the…

A: pH of resulting solution will depend upon nature of resulting solution either acidic or basic.

Q: What is the volume of 0.20 M NaOH that would be needed to reach the equivalence point with 30.0 mL…

A: Equivalence point is defined as the point at which the amount of titrant is added to the analyte…

Q: What is the final pH of a solution made by mixing 100 mL of 0.05 M CH3COOH and 100 ml of 0.1 M…

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

Q: HF is a weak acid. If a solution of HF with a pH of 4.5 is made, Which of the following would be the…

A:

Q: 15. The table below shows the color of the indicators methyl orange nd litmus in two samples of the…

A: Methyl orange is an indicator which shows red color when pH<3.1 and shows yellow color when…

Q: what is the pH of a solution made by mixing 15.00 mL f 0.2M sodium hydroxide with 15.00 mL of 0.2M…

A:

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: 7) 150.0 mL of 2.50 M NaOH is added to a 200.0 mL solution of 1.80 M HF. Assume that the volumes are…

A: HF        +     NaOH→    NaF    +     H2O1.80M           2.50M200ml           150mlno. of moles of…

Q: You are titrating 50 mL of 0.100 M HF with 0.050 M NaOH. What is the pH after: a. 50 mL of NaOH…

A: Since we know that  pH = - log [H+] From given solution first of all we find the concentration of…

Q: When 50 mL of 0.20 M ammonium nitrate and 50 mL of 0.10 M calcium hydroxide are combined, the pH of…

A: Volume of ammonium nitrate solution= 50 mL  Concentration of ammonium nitrate solution = 0.20 M…

Q: 201 Calculate the pH of the resulting solution When 20.0 mL of 6).150M NaOH is added to 500mL of…

A:

Q: A solution that contains a weak acid and its conjugate base in roughly equal concentrations is A.…

A:

Q: A solution is made by mixing 0.400M in formic acid, HCOOH, and 1.00M in sodium formate, HCOONa?…

A: Given -> Molarity of formic acid= 0.400 M Molarity of sodium formate = 1.00 M Ka = 1.80 × 10-4…

Q: Calculate the pH of the following solutions. a) 0.400 M HCl solution  b) Solution containing 0.727…

A: Formula: pH = -log[H+] pH = pKa + log[salt]/[acid] pH = 7 + (pKa + logC)/2

Q: 11. Ifa buffer solution is made from 300.0 ml of 1.6 M aniline salt mixed with 250.0 ml of 2.0M…

A: When a weak base and its salt are present in a solution, they form buffer solution.pH of such a…

Q: 1. Which of the following is true for a buffered solution?  a. The solution resists change in its…

A:

Q: Calculate the after adding 10.00 mL of 0.15 M HCl to 50 mL of pure water b. Calculate the pH after…

A: for dilution  M1v1=M2V2  M1 =molarity before dilution V1=volume acid/base  M2 = molarity of solution…

Q: 6. A titration is carried out where 3.0 mL of 0.70 M NaOH is added to 15.0 mL of 0.150 M HCl. What…

A: Given, For NaOH solution Concentration of NaOH solution = 0.70 M = 0.70 mol/L Volume of NaOH…

Q: Which of the following procedures will create a buffered solution? ii. i. Equal volumes of 0.5 M…

A:

Q: 2. How many moles of HOCI should be present together with 0.50 mole of Ca(OCI)2 in a 1.00 L solution…

A: Step 1:Step 2:Step 3:Step 4:

Q: Calculate the pH of a solution containing 200ml of 0.01M Acetic acid and 80ml of 2.5M sodium acetate

A:

Q: Calculate the change in pH that occurs when 1.0 g NaOH is added to 250 mL of each of the following…

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…

Q: What is the pH of a solution made by mixing 40.0 mL of 0.20 M HCl with 40.0 mL of 0.10 M KOH?…

A: HCl and KOH will react as per the following reaction HCl + KOH --> KCl + H2O

Q: A student dissolves a sample of a weak acid, HA, in 20.0 ml of H;O. The student then takes 5.6 mL of…

A: Given, Volume of water = 20.0 mL Volume of sample = 5.0 mL pH of final solution = 4.5

Q: When 25.0 mL of 0.200 M hydrochloric acid and 25.0 mL of 0.200 M potassium cyanide are combined, the…

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

Q: How many grams of lactic acid and mL of 0.1M sodium hydroxide must be added to 100 mL of water to…

A:

Q: Which of the following pairs of substances can be used to make a buffer solution?   a. HBr & KOH…

A: A multiple choice question based on buffer solution, which is to be accomplished.

Q: Calculate the pH of the solution formed by mixing 25.0 mL of 0.200 M NaH2PO4 with a. 25.0 mL of…

A:

Q: A solution is prepared by mixing 10mL of 1 M HCI and 10mL of 1.2 M NaOH. What is the pH of the…

A:

Q: If a buffer solution is made from 450.0 mL of 3.8 M aniline salt mixed with 400.0 mL of 4.1 M…

A:

Q: 0.95

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.