Choose the correct answer from the choices below

sing the Brønsted-Lowry concept of acids and bases, identify the Brønsted-Lowry acid and base in each of the following reactions

miskamm [114]

Answer: a) $HSO_3^-$ : Bronsted base

$H_2O$ : Bronsted acid

b) None

Explanation:

According to the Bronsted-Lowry conjugate acid-base theory, an acid is defined as a substance which looses donates protons and thus forming conjugate base and a base is defined as a substance which accepts protons and thus forming conjugate acid.

For the given chemical equations:

a) $HSO_3^-(aq.)+H_2O(l)\rightarrow H_2SO_3(aq.)+OH^-(aq.)$

Here, $HSO_3^-$ is accepting a proton, thus it is considered as a base and after gaining a proton, it forms $H_2SO_3$ which is an conjugate acid.

And, $H_2O$ is losing a proton, thus it is considered as a acid and after losing a proton, it forms $OH^-$ which is a conjugate base.

b) [tex[(CH_3)_3N(g)+BCl_3(g)\rightarrow (CH_3)_3NBCl_3(s)[/tex]

As there is no donation or acceptance of $H^+$ , they cannot be considered as Bronsted acid or base. $(CH_3)_3N$ gives its electrons to $BCl_3$ , thus $(CH_3)_3N$ act as lewis base and $BCl_3$ act as lewis acid.

6 0

3 years ago

At its triple point, water can

garik1379 [7]

A exist in equilibrium in three different phases

4 0

3 years ago

Read 2 more answers

(4x2 + 5x) - (7x - 3x2 + 1)

Tanya [424]

Answer:

7x2−2x−1

Explanation:

do u need the explanation if so ill add it

8 0

3 years ago

By definition, a(n) _______acid is any species that can donate a proton. Ammonia has a proton bonded to nitrogen, so ammonia can

pochemuha

Answer:

A Brønsted-Lowry acid.

A Brønsted-Lowry base.

Ammonia is an acceptor of proton.

Explanation:

A Brønsted-Lowry acid is any atom that can donate a proton (H +) to another atom or molecule whereas Brønsted-Lowry base is any species that can accept a proton from another atom or molecule or in other words, a Brønsted-Lowry acid is a proton donor, while on the other hand, a Brønsted-Lowry base is a proton acceptor. The ammonia molecule accepts the hydrogen ion is considered as the Brønsted-Lowry base.

5 0

3 years ago

Rank and explain how the freezing point of 0.100 m solutions of the following ionic electrolytes compare. List from lowest freez

Elden [556K]

Answer:

The solutions are listed from the lowest freezing point to highest freezing point.

Mg₃(PO₄)₂ - AlBr₃ - BeBr₂ - KBr

Explanation:

Colligative property of freezing point, is the freezing point depression.

Formula is:

ΔT = Kf . m . i

Where ΔT = T° freezing pure solvent - T° freezing solution

Kf is the cryoscopic constant

m is molality and i is the Van't Hoff factor (number of ions, dissolved in solution)

In this case, T° freezing pure solvent is 0° because it's water, so the Kf is 1.86 °C/m, and m is 0.1 molal.

The i modifies the T° freezing solution. The four salts, are ionic compounds, so for each case:

BeBr₂ → Be²⁺ + 2Br⁻ i = 3

AlBr₃ → Al³⁺ + 3Br⁻ i = 4

Mg₃(PO₄)₂ → 3Mg²⁺ + 2PO₄⁻³ i = 5

KBr → K⁺ + Br⁻ i = 2

Solution of Mg₃(PO₄)₂ will have the lowest temperature of freezing and the solution of KBr, the highest (always lower, than 0°).

8 0

3 years ago