Show the reaction of HF (weak acid)  with water:

Q: Calculate 3OH-4 and pH for each of the following strong base solutions: (a) 0.182 M KOH

A:

Q: Explain which is the stronger acid a)HNO, or HCIO. b) CH;FCOOH and CH;BrCOOH

A: Acid: A substance that donates proton is treated as acid.  A substance that has more tendency to…

Q: 4) How would you explain the difference between a weak acid (like HF) and a strong acid (like HNO3)?

A: Weak acids are HF, CH3COOH etc. Strong acids are HCl, HNO3 etc.

Q: Calculate [OH-] given [H3O+] in the aqueous solution. [H3O+]=3.3*10^-3 M

A: pH of the solution is given by,                               By using given concentration to get…

Q: What is the pH of a solution with a [H+] = 0.001 M? 4 13.999 3

A: Given that, [H+]=0.001M so,

Q: The pOH of a solution is 3.72. What is the OH¯ concentration in the solution?

A: We know that pOH is related to the OH- concentration by the following equation: pOH = - log10[OH-]…

Q: What acid and what base would react with CsNO3

A: Given salt for formation is CsNO3

Q: What is the experimental enthalpy (in kJ/mol) for the neutralization reaction between HX and NaOH?…

A:

Q: What is pH of H2SO4 solution of 10 mg/L?

A: pH :-        It is a scale to measure the acidic or basic property of any substance . That tells…

Q: If 0.0750 moles of barium hydroxide were added to water, how many moles of OH- would be produced?…

A: Given, Chemical formula of barium hydroxide - Ba(OH)2 Moles of barium hydroxide, Ba(OH)2 = 0.0750…

Q: For a given aqueous solution, if [OH-]=1.0x10^-12 M what is [H+]

A: For the aqueous solution, the concentration of the hydrogen ion and hydroxide ion is constant at a…

Q: Calculate AH for the reaction CH4 (g) + NH3 (g

A:

Q: Calculate the pH of 0.02 M H;PO4

A:

Q: The pOH of a solution is 3.43. What is the OH" concentration in the solution?

A:

Q: HBr OH

A: The given reaction is the conversion of tertiary alcohol with HX acid to the alkyl halide.…

Q: CO,H OH (34) COOH

A: In this reaction we will find out the element or functional group present next to the alkene in the…

Q: What is the pH of an HCl solution if [H+] = 0.03? A. 0.03 B. 1.5 C. 3.0 D. 3.5

A: Given that : [H+] = 0.03 pH of the HCl solution = ?

Q: The following is a property of acids, bases, or neither ? Produce CO2 from NaHCO3

A: The following is a property of acids, bases, or neither ? Produce CO2 from NaHCO3 A. acids B. bases…

Q: 1. NAOH, H2O 2. H300 i. NaOEt ii. MeBr 3. heat Ph OEt

A: Applying concept of organic synthesis.

Q: Calculate [H'] and [OH] for solutions with the following pH values: a) 4.0 b) 8.52 c) 12.60

A: The concentration of hydrogen ions in an aqueous solution is measured in pH scale. Mathematically,…

Q: 3. Calculate the value of [H3O*] from the given [OH ]in each solution and label the solution acidic…

A: pH  of any solution is expressed as the negative logarithm of hydrogen ion or hydronium ion…

Q: 1. Calculate [H] and [OH] for solutions with the following pH values: a) 4.0 b) 8.52 c) 12.60

A: given a) pH = 4 b) pH = 8.52 c) pH = 12.60

Q: Calculate the pOH of a solution  with [OH-]  = 4.5x 10 -14 M

A:

Q: What is the pOH of a 0.43 M KOH solution?

A:

Q: Calculate the pOH of a solution with [OH-] = 6.8 x 10-9 M

A: Given  ; [OH-] = 6.8 × 10-9 M  To calculate the pOH of the solution.

Q: Calculate the pOH of a solution with [H+]= 1.4 x 10^-9 M.

A: Given: [H+]= 1.4 x 10-9 M

Q: How much more H+ is in water at a pH of 3 when compared to a pH of 6?

A: The equation relating pH and concentration of H+ is given below.

Q: if the pOH is 3.09 what is the pH?

A: If pH is less than 7 then solution is acidic in nature.If pH is greater than 7 then solution is…

Q: How many milliliters of 0.258 M NaOH are required to completely neutralize 2.00 g of acetic   acid…

A:

Q: Calculate OH- and H3O+ in 3.0 x 10^-2 M NaOH, using Kw

A: The solution is as follows :

Q: Given the pOH = 8.7, find the [OH-] concentration

A: The conversion formula for pOH and [OH-] is pOH=-log [OH-]  [OH-]=10-pOH ​

Q: What is the [H+] concentration of a solution with a pOH of 5?

A:

Q: A dilute solution of hydrochloric acid (HCI) ha

A: pH of solution gives the hydrogen ion concentration which tells about the acidity of solution. pH is…

Q: What is the [H*] and pH of a sample with [OH] = 1 x 105?

A: Given,  [OH-] = 1 × 10-5 We know that  [H+][OH-] = 10-14

Q: {OH-} =0.002 M  pH=

A:

Q: How many moles of NaNO3 is formed if 20 mL of 0,1M HNO3 is needed to neutralize a solution of NaOH

A: Given  Volume of HNO3 = 20 mL Concentration of HNO3 = 0.1 M So, No of moles of HNO3 used = volume ×…

Q: pH and pOH of [H+] = 4.02×10-8 M

A:

Q: g acid base reactions

A: 1.     In the first case NaOH is strong base and it easily removed H+ from phenol, so the reaction…

Q: Calculate [H3O+] when pOH is 8.90  Calculate the pH of an NaOH solution where [OH-] = 4.6 x 10-5

A: Concentration of H3O+ can be calculated as follows:

Q: What is the pOH of a solution at 25 oC when the pH is 5.42?

A: Given,    Temperature = 25◦c     pH = 5.42     pOH =?

Q: Calculate the pH of a solution with [H,O*] of 8.96×10 4 pH =

A:

Q: pOH of 10.81 What is the Molarity of hydroxide ions in the solution?

A: Inorganic chemistry.

Q: Will a solution whose [H] = 5.04 x 10 be acidic, basic or neutral?

A: Given : Concentration of H+ ions=5.04×10-3  To identify : The nature of solution

Q: Det 2 Hy0 ELoh 2. ich 3.H30°, heat Ph

A: In presence of acid or base, carbonyl compound having enolisable alpha Hydrogen undergo reaction by…

Q: What is the pH of a 0.050 M solution of formic acid?

A:

Q: What is the pH of a 0.0235 M H* solution?

A: pH :-  It is defined as , the negative logarithm to the base 10 of hydrogen ion concentration…

Q: pH= 7.9; calculate [H+]

A: pH of a solution is a negative logarithm of Hydrogen ion (or hydronium ion) concentration. It stands…

Q: HF is a weaker Brønsted acid than HI and a stronger acid than H2O.

A: Brønsted acid = Compound that donates hydrogen ion or we can say that transfer Hydrogen ion Compound…

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.