Based on the pH measured for the solution of (NH4)2CO3, is NH4+ is a stronger acid or is CO2−3 stronger base? and Why?

Q: (a) Give the conjugate base of the following Brønsted–Lowry acids: (i) HIO3, (ii) NH4+. (b) Give the…

A: Conjugate base :  the conjugate base is able to gain a proton in a chemical reactio     Conjugate…

Q: If the Kb for hydrazine, N2H4(aq), is 1.7 x 10-6 , calculate the pH of a 1.8 mol/L solution of…

A: To calculate the pH of a 1.8 mol/L solution of hydrazine.  Given: Kb for hydrazine, N2H4(aq) = 1.7 x…

Q: The pH of a solution containing a [H3O+] = 3.40 x 10 negative 5 M, is:

A: pH is a scale to measure the concentration of hydrogen ions. The negative logarithm of hydrogen ion…

Q: Calculate the pH of a 0.050- M Al(NO3 )3 solution. The Ka value for Al(H2O)6 3+ is 1.4 × 10−5.

A: The question is based on the concept of chemical equilibrium. we have to calculate pH of the…

Q: Calculate the pH of a 0.600M solution of tin chloride SnCl2.

A:

Q: Why is (CH3)3Cl considered to be a Lewis Acid?

A: The Lewis concept of acid and bases is the most accepted definition which is used to explain the…

Q: What is the pH of a 1.278 M NaH2AsO4 solution

A: There are two types of bases/acids. One is strong base/acid which is completely dissociable into its…

Q: a) Arrange the following ions in order of increasing acidity in aqueous solution: Fe3+. Na+, Mn2+.…

A: Fazan's rule helps to determine whether the compound is ionic or covalent. The postulates of Fazan's…

Q: Calculate the pH of a 0.022 M RbOH solution.

A:

Q: Explain the steps to determining the presence of Pb2+ ions.

A: We know that Pb2+ ion is group 1 ion. The steps to determine the presence of Pb2+ ion are given in…

Q: Calculate the pH and the pOH of these solutions:   (c) 0.957 M HC2H3O2 (Ka = 1.8 x 10-5) pH =   pOH…

A:

Q: What is the pH of a 0.820 M solution of Ca(NO₂)₂ (Ka of HNO₂ is 4.5 × 10⁻⁴)?

A: The pH of the solution is equal to the negative logarithm of hydronium ion while pOH of the solution…

Q: What will be the pH of a solution containing 0.200 M NaH2PO4 and 0.200 M Na2HPO4? Ka(NaH2PO4) = 6.2…

A: Given,  Molar concentration of weak acid, NaH2PO4 or H2PO4- = [H2PO4-] = 0.200 M Molar concentration…

Q: Ammonia, NH3, is amphoteric. (a) Give the formula for the conjugate acid of NH3. (b) Give the…

A: Write conjugate acid and conjugate base of NH3 ---

Q: The acid ionization constant for Al(H2O)63+(aq) is 7.9×10-6. Calculate the pH of a 0.0348 M solution…

A:

Q: What is the conjugate base of boric acid, B(OH)3?             (A) OH–            (B) B(OH)4–…

A: According to Bronsted concept , acid is a substance which donates proton and base is the substance…

Q: The fluoride ion reacts with water to produce HF. Is fluoride acting as a Lewis acid or as a Lewis…

A:

Q: A weak acid, HA, has pKa=6.2. If a solution of NaA (aq) is prepared, what does the pH of the…

A: The Henderson–Hasselbalch equation relates the pH of a solution containing a mixture of the two…

Q: Calculate K₂ or K from experimental data. The pH of a 0.14-M solution of chlorous acid (HCIO₂) is…

A: Since you have posted multiple questions ,we will provide the solution only to the first question as…

Q: Calculate the pH of a 0.100 M HC2H3O2(aq) solution.

A: The acid in the given problem is depicted by the formula C2H3O2H is acetic acid . It can be written…

Q: hat is the equilibrium constant expression for the following reaction?   2 NaHCO3 (aq) ⇌ Na2CO3…

A: Let , consider a general reaction aA +bB →cC +dDThe equlibrium constant  in term of…

Q: Calculate the pH of a 0.1M solution of protonated methylamine (pKa =7)

A:

Q: What is the pH of a 0.950 M solution of Na2HPO4? H3PO4 is a weak polyprotic acid with Ka1 =…

A: The objective of this question is to calculate the pH of a 0.950 M solution of Na2HPO4. The compound…

Q: A weak acid, HA, has a pKa = 6.2.  If a solution of NaA(aq) is prepared, what does the pH of the…

A:

Q: (4) Which acid below would have a stronger conjugate base? Give the reason (a) HCN, Ka=6.2 x 10-10…

A:

Q: Predict the direction for the reaction and explain. [CuI4] (aq) −2 + [CuCl4] (aq) −3 ⇌ [CuCI4] (aq)…

A:

Q: Calculate the PH and POH for a .008 Moles solution of HC2H3O2  and .01 Moles in KC2H3O2

A: Answer: Buffer solution is a type of solution that resists the change in its pH on adding small…

Q: Determine the pH of a 0.100 M solution of (NH4)2C2O4.

A: The reaction for the above process can be written as : (NH4)2C2O4 + H2O ------> 2NH4+  +C2O4^2-…

Q: What is the conjugate acid of potassium hydrogen phosphate, K2HPO4?

A: K2HPO4 is a base. Its conjugate acid can be obtained by adding a hydrogen atom to it. The net ionic…

Q: Calculate the pH of the solution in which 0.2M NH4Cl and 0.1M NH3 are present. The pK of ammonia…

A:

Q: calculate the ph of the following solutions:   0.1 M solution of the salt CaF2 where the pKa(HF) =…

A:

Q: The acid ionization constant for Sc(H2O)63+ (aq) is 5.0×10-5 . Calculate the pH of a 0.0043 M…

A: Given , acid ionisation constant , Ka= 5.0×10-5 concentration of the Sc(NO3)3= 0.0043 M

Q: What is Ka for the conjugate acid of NH₃ (Kb = 1.8 × 10⁻⁵)?

A:

Q: rite the balanced equation that accounts for the source of OH- used in the following reactions:…

A: the balanced equation are as follows:

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.