1. Complete both questions: a. Prove that HSO4- can act as an amphoteric substance. b. Explain why...

1. Complete both questions: a. Prove that HSO₄^- can act as an amphoteric substance. b. Explain why CH₄ cannot act as an amphoteric substance.

2. Try this question again. Be sure to use claim-evidence-reasoning when you format your answer and be sure to show your work for any calculations performed to develop your evidence. Which is more dangerous if you spill it on your hand a 0.025 M HBr solution (Ka = 1.3 x 10⁶ ) or 0.75 M HClO₂ solution (Ka = 1.2 x 10^-2 )?

3. For each pair below indicate which is stronger and support your answer with an explanation. a. Which is a stronger acid, H₂S or PH₃? b. Which is a stronger base CO₃^-2 or C₂H₅O^-?

4. Calculate the equilibrium concentration of NO in the reversible reaction below using the initial concentrations given for each reactant and product. The equilibrium constant for the reaction is Kp = 20. 2 NO (g) ⇌ N2 (g) + O2 (g) Initial concentrations: [N2] = 0.5 atm, [O2] 0.5 atm, [NO] = 0.75 atm

Solutions

Expert Solution

Solution to question 1:

A substance which is acting as both an acid and a base are called amphoteric in nature. That means it will be able to donate as well as accept protons.

a. HSO4- is amphoteric - Explanation:

It can lose the proton to become a sulfate ion in a basic environment.

HSO4- + B- HB + SO42-

It can accept another proton to become H2SO4 in an acidic environment.

HSO4- + H+ H2SO4

HSO4- accepts as well as donates protons when required depending upon the environemnt. Hence it is an amphoteric substance.

b. CH4 is not amphoteric - Explanation:

H2O can donate proton more readily than CH4 because O atom is more electronegative than C atom . Hence the acidity is far less for CH4. Further, it cannot accept a proton and form highly unstable CH5+ ion. Hence CH4 cannot act like an amphoteric substance.

queen_honey_blossom answered 8 months ago

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