A solution with an OH| concentration of 1.20×10-7M has a pH of O 7.06 O 7.07 O 7.08 7.09

Q: Calculate the [OH- and the pH of a solution with an [H*] = = 6.8 x 10-10 M at 25 °C. [OH]= %3D pH =…

A: The answer to the given three questions can be answered as follows -

Q: How many gram of ammonia should be added to 500mL of 1M ammonium chloride to give a pH 9? Ka…

A:

Q: 9) Classify each of the following acids as strong or weak. If the acid is weak, write an expression…

A:

Q: How many grams of NH4Cl (53.49 g/mol) must be dissolved in 0.639 L of solution in order to obtain a…

A: we need to find mass of NH4Cl in the solution for a pH 4.79

Q: What is the pH of a 0.100 M NaCN solution. K, of HCN at 25°C is 6.2 x 10-10. O 11.10 O 5.10 O 8.89 O…

A: Given data,Molarity=0.100MKa of HCN=6.2×10-10

Q: An aqueous solution has a hydrogen ion concentration of 1×10-13 M   (10 -13 M). (1) What is the…

A: Given: H3O+=1×10-13 M Formula used:pH+pOH=14

Q: 4.0 g of baking soda (NaHCO3 , 84.02 g/mol) is fully dissolved in 100.0 mL water.  What is its pH?…

A: NaHCO3 is an amphiprotic species. That is, it can act as acid as well as a base.  The pH of such…

Q: Complete the following table by calculating the missing entries.In each case indicate whether the…

A: The equations which are useful to solve the above problem are  1) pH + pOH = 14  2) pH = -log[H+] 3)…

Q: What is the pH of a 0.250 M HOCI solution? K, of HOCI at 25°C is 3.5 x 10-8. O 7.46 O 4.03 O 3.57 O…

A: ​Given - - - >   Ka = 3.5*10-8   pH = 0.25

Q: Consider a 1.0 L of 0.1 M aqueous solution consisting of weak acid HA, which has K₂ = 3.9 x 10-4, at…

A: HA is a weak acid that is very weakly dissociated to give H+(aq) ions. HCl is a very strong acid…

Q: The acid ionization constant for Pb(H2O)62+(aq) is 6.3×10-7. Calculate the pH of a 0.0538 M solution…

A:

Q: Calculate the [OH-] and the pH of a solution with [H] = 3.0 x 10 Mat 25 °C. [OH-] = [H*] = Calculate…

A: The objective of the question is to calculate the concentration of hydroxide ions and the pH of a…

Q: Question Aniline, C6H5NH2, is a very weak organic base that is used in the production of…

A:

Q: The pyridinium ion (C5H4NH*) is a weak acid (Ka = 5.60 x 10-6). Calculate the pH of a solution that…

A: Given that, the pyridinium ion is a weak acid. The Ka of it is Ka = 5.60×10-6. 3.7 mL of 0.167 M of…

Q: Which of the following reactions are acid-base reactions? Cu2+ + Zn ⟶ Cu + Zn2+ NaCl ⟶ Na+ + Cl-…

A: According to Bronsted-Lowry concept of acids and bases  Acid is a species which can donate a proton…

Q: Consider the following data on some weak acids and weak bases: name nitrous acid acid hydrofluoric…

A: Answer:Two concepts will be required to arrange the given solutions in increasing order of pH:Salt…

Q: the pH and concentrations of species the following sõlutions (a) 0.20 M K,HPO4 An amphiprotic…

A: Amphiprotic species   Amphiprotic species can act both as acid and base by donating or accepting…

Q: "Vhen 4.73 g of the weak acid HC6H4CIO is dissolved in 800 mL of olution, he pH is 5.25. What is the…

A: Ka is acid dissociation constant.

Q: Which of the following statements is true? a basic solution has an H3O* concentration greater than…

A: Understanding the characteristics of acidic and basic solutions is fundamental to the study of…

Q: Sodium hydrogen sulfate (NaHSO4) which dissolves in water to release H+ is used to adjust the pH of…

A: ppm is used to express the concentration of solution

Q: Aspirin, which is acetylsalicylic acid, is the most common over the counter pain killer. Over 15…

A: POH= -log[OH-] =-log(4.4*10^-12) =11.36

Q: If 0-2 pH is considered strongly acidic, 2-7 is weakly acidic, 7.0 is neutral, 7-12 is weakly basic…

A: pH is basically defined as negative log of concentration of H+ ions.  The correct explanation and…

Q: Which of the following statements is true?   a basic solution has an H3O+ concentration greater…

A: Understanding the relationship between hydroxide ion concentration, pH, and the alkalinity of a…

Q: pH is a logarithmic scale used to indicate the hydrogen lon concentration, [H], of a solution: pH =…

A: Given :  For part A :  Mass of HCl = 0.55 g  Volume of solution = 5.5 L   For part B :  Mass of NaOH…

Q: Can you please answer question 3

A: The question is based on the concept of the pH of the solution. It is defined as a negative…

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.