" in .25M represents what?   Question 4 options:   Concentration   None of the above   Color   pH

Q: calculate the

A: Ammonium chloride (NH4Cl) is salt of weak base-strong type. pKb of weak base = 4.74 Concentration of…

Q: when the ratio of (A--)/(HA)=100 to 1, calculate the pH. when the ratio of (HA)/(A--)=10 to 1, the…

A: We have to give the pH for given conditions.

Q: The ph of an unknown solution is 8.84. Calculate the pOH. Express your answer in standard notation…

A: pH of the solution depends on concentration of H+ ion present. With increase of H+ ion…

Q: When weak acids such as and are diluted with deionized water, their pH When weak bases such as are…

A: Weak acids are the species that give H+(aq) ion in water and are very weakly dissociated in water.…

Q: When a strong base is added to a solution with pH of 7.5, the pH of the solution will A.) Increase…

A: A solution with pH = 7.5  we have to determine what will happen if a strong base is added to that…

Q: Calculate the pH of each solution given the following. [H3O+]=9×10−6M  Express your answer using…

A:

Q: please indicate next to each item if acid, neutral or basic

A: pH and hydronium ion concentration, [H3O+] are related as, pH = - log ([H3O+])

Q: A 0.0015 M solution of a weak base has a pH of 9.84. Calculate Kb

A: We have given that pH of Weak base = 9.84 Concentration of Weak base = 0.0015M pH + pOH = 14 pOH =…

Q: Calculate the pH of each solution given the following. [OH−]=8.7×10−6M  Express your answer using…

A: Given: Concentration of OH- is  8.7×10-6 M. To find: pH

Q: If a neutral acid donates a proton, the conjugate base will have a charge of _______. Type both an…

A: Neutral acid:

Q: State whether each of the following solutions is acidic, basic, or neutral. a.[H3O+]=5.6×10−10M…

A: We have four concentration of hydrogen ion , we have to predict whether solution will be acidic,…

Q: Calculate the [H3O+] using the equation that relates the concentration to the inverse log of the…

A:

Q: When some amount of KOH is added to a solution of ammonium hydroxide, Kb for ammonium hydroxidewill…

A:

Q: I. Calculate pH from the following hydrogen ion concentration (M). Identify each as an acidic pH or…

A: Since you have asked multiparts questions, we will solve the first three sub parts questions for…

Q: Complete the following table with the needed [H3O+], [OH-],  pH, and pOH. Then, classify the…

A: Complete the following table with the needed [H3O+], [OH-],  pH, and pOH. Then, classify the…

Q: Q2: Calculate the pH of a 1.3 * 10 ^ - 9 M HBr solution ?

A:

Q: I Review | Constants Assuming each solution to be 0.10 M, rank the following aqueous solutions in…

A: The order of pH is

Q: A 1500 L spill of a strong acid that donates one proton has occurred on the side of a highway when a…

A: pH is used to determine the acidity or alkalinity of a solution. The pH is determined as the…

Q: b) Which is a reasonable pH for vinegar (sour taste)? 4; 7; 9; 12

A: pH is defined as the negative logarithm to the base 10 of hydrogen ion concentration  expressed in…

Q: What is the pH of a solution of HCL in which (HCI] = 2.6 x 10 M7 (2 decimals only)

A:

Q: mist dissolves 845. mg of pure hydroiodic acid in enough water to make up 70. mL of solution.…

A: Given, amount of hydroiodic acid =845 mg =0.845 garmvolume of solution =70 mL =0.07 Lwe are asked to…

Q: Calculate the pH of the solution, after you add a total of 53.8 mL 0.200 M HNO3. Express your answer…

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

Q: Calculate the pH of the following given the molar hydrogen ion concentration. A. Carrots,…

A: Used Formula- pH=-log[H^+] [H^+]=9.4×10^-6M

Q: Determine which polyprotic acid from the list is the unknown acid.

A:

Q: Which of the following is correct concerning the acid ionization constant, Ka, of iodous acid, HIO2?…

A: The question is based on the concept of acidity. It is measured in terms of acid dissociation…

Q: Fill in the missing chemical formulae in the tables below. conjugate acid conjugate base HCO, "oa'H…

A:

Q: weak acids. Use the Ka values in the following table to help answer some of the questions. a) Using…

A: In the given question we have to predict which one of the acid has lowered pH and acidic by using…

Q: Calculate [H3 0+] for a solution with a pH of 9.85. Express the concentration using two significant…

A:

Q: 1. Draw the pH scale from 0 to 14. 2. Indicate where on the scale it  is acidic and basic and…

A:

Q: Part C Calculate the pH of a 0.20 mol L-1 solution of KCN. Express the pH numerically to two decimal…

A: Here, we have to find the value of pH for the given concentrations of particular salts.

Q: alculate the [H+][H+] and pH of a 0.00250.0025 M iodoacetic acid solution. The ?aKa of iodoacetic…

A:

Q: Complete the following table with the needed [H3O+], [OH−], and pH, and classify the solution as…

A: Given: Table  To find : complete the given table Solution: If the pH range is less than 7 then it is…

Q: A certain weak base has a ?b of 7.50×10^-7. What concentration of this base will produce a pH of…

A:

Q: ntify if each beaker is a strong acid, weak acid, strong base or weak base. Explain in detail using…

A: pH is a quantitative measure that how the given aqueous solution is acidic or basic. The pH range is…

Q: Calculate the pH of each solution given the following. [H3O+]=4.5×10−2M Express your answer…

A: The pH of a solution is determined by taking the negative logarithm of hydrogen or hydronium ion…

Q: Human blood has a normal pH range of 7.35 to 7.45. The range seems fairly small in terms of pH but…

A: The Ph scale is logarithmic and inversely indicates the concentration of Hydrogen ions in the…

Q: If the following salt was dissolved in water, select whether the cation and anion would be acidic,…

A: Salts that on dissolving make the solution acidic are called acidic salts. On the other hand, we…

Q: An 8.0 mass percent solution of H3PO4 in water has a density of 1.0465 g/mL. Calculate the pH, the…

A: Given data : An 8.0 mass percent solution of H3PO4 in water has density = 1.0465 g/mL. Calculate…

Q: If the pH of a solution is 3.3, then the pOH is [ Select ] and the solution is [Select ]

A: Given that, PH of solution=3.3 POH=? nature of Solution=?

Q: Draw the pH scale (with correct numerical reference). Label where acids, bases, neutral substances…

A: PH is defined as the negative logarithm of the H+ ion concentration. It was introduced by Sorensen.…

Q: Classify each salt as acidic, basic, or neutral. Drag the appropriate items to their respective…

A: Acidic salt: Produces strong acid and weak base after hydrolysis Basic salt: Produces weak acid and…

Q: A chemist dissolves 793. mg of pure hydrobromic acid in enough water to make up 90. mL of solution.…

A: Given data,Mass of HBr=793mg=0.793gVolume of solution=90mL=0.09L

Q: Calculate the pH of a 0.400M solution of quinoline, C₉H₇N.

A:

Q: I. Calculate pH from the following hydrogen ion concentration (M). Identify each as an acidic pH or…

A: Note: As per our guidelines, we are supposed to answer only three subparts. Please repost the…

Q: What pH levels are neutral? Acidic?  basic?

A: pH is a measure of how acidic / basic any solution is. it's range is from 0-14 neutral range is 7 .…

Q: A certain weak base has a K, of 7.20 × 10-7. What concentration of this base will produce a pH of…

A: Given  Kb = 7.20 x 10-7 pH = 10.14  we know  pH + pOH = 14  pOH = 14 - 10.14 = 3.86 and   [OH-] =…

Q: hat ph and %ionization of 0.100M arsenic acid H2AsO4

A: The pH scale is used to rank solutions in terms of acidity or basicity (alkalinity). Since the scale…

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.