Differentiate between the serms sarengrh and concentration as they apply to acids and bases. Whe

step 1 So strength is the property of an acid molecule itself. So strong acids dissociate completely in

Differentiate between the serms sarengrh and concentration...

Key Concepts

Acid and Base Strength vs Concentration

Strength refers to the degree to which an acid or base dissociates or ionizes in water, whereas concentration is about how many moles of the substance are present per unit volume of solution. A strong acid or base completely dissociates regardless of its concentration, while a weak one only partially dissociates. Concentration, on the other hand, pertains solely to the amount of substance, independent of its inherent ability to ionize.

Strong Acid and Weak Acid

A strong acid, such as HCl, dissociates completely in water, meaning nearly all its molecules release protons, regardless of whether the solution is dilute or concentrated. A weak acid only partially dissociates, meaning that in solution only a fraction of the acid molecules donate their protons, which affects both its reactivity and equilibrium properties.

Properties of HCl

Hydrochloric acid (HCl) is intrinsically a strong acid because it ionizes completely in water. This characteristic holds true over a wide range of concentrations. When HCl is at a high molarity, the solution is said to be concentrated, meaning there are many moles of acid per liter; when it is at low molarity, the solution is dilute, meaning fewer acid molecules are present. In both cases, however, HCl remains a strong acid because of its complete ionization.

Properties of Ammonia

Ammonia (NH3) is a weak base because it reacts with water to form ammonium ions and hydroxide ions but does not completely convert into these ions. Similar to acids, the concentration of ammonia (whether concentrated or dilute) refers to the amount of ammonia present in the solution, while its property of being a weak base stems from its limited ionization in water.

Conjugate Acid-Base Pairs

In acid-base chemistry, every acid has a conjugate base, and every base has a conjugate acid. The conjugate base of a weak acid is generally stronger than the conjugate base of a strong acid, because a weak acid does not release its proton as readily, leaving its conjugate base relatively more eager to accept a proton. However, being 'stronger' in this context does not necessarily mean it is a strong base; it simply has a greater tendency to accept a proton compared to the conjugate base of a strong acid.

Transcript

00:01 So strength is the property of an acid molecule itself.

00:05 So strong acids dissociate completely in solution.

00:10 So if you have an acid hx, for example, and we put it in solution, so we add it to water, it completely dissociates into hydronium h3o plus and the anion x minus.

00:27 And so we don't have any hx remaining.

00:31 We just have h3o plus and x minus in solution.

00:36 Weak acids do not fully dissociate.

00:39 So the same hx plus h2o, you would have an equilibrium with hydronium and x minus.

00:50 And so equilibrium just means that we still have, just to do the states here.

00:56 So this is acreous liquid.

01:03 These are aqueous.

01:05 And so it means that we still have some of the acreous molecule still intact here.

01:13 So instead of 100 % associating, it might be 5%, 10%, could be as little as 1%.

01:22 But we still observe the h3o plus and therefore a ph change.

01:28 And so if we look at an example, hcl is a strong acid because when we add it to water, we get hydronium and x minus, there's no hcl molecule left fully intact.

01:44 All of the hcl bonds have broken.

01:47 And so this means that the concentration of h3o plus is going to be equal to the concentration of hcl that you added.

01:56 So if you added one mole of hcl to one liter of solution, you've created a one molar solution of hcl.

02:07 Since it fully dissociates, you're going to have a one molar solution of h3o plus.

02:14 So weak acids, for example, hf, don't fully dissociate.

02:21 So we have an equilibrium, h3o plus and f minus.

02:28 So the concentration of f minus resulting is going to be much less than the concentration of hf that you added.

02:37 And that's also true for the h3o plus.

02:45 And then just to balance everything out, concentration of cl minus would be equal to h3o plus on this side and hcl.

02:56 Here, let's say you added one mole of hf to one liter of water, the concentration of h .jo plus might be 0 .05.

03:10 It's less than one molar.

03:13 This would be the same.

03:15 So it doesn't fully dissociate.

03:17 So there's still a lot of hf molecule intact in solution.

03:22 So if we were to look at solutions, this is when we get.

03:30 Into concentrated and dilute.

03:34 So acids and bases have strength.

03:38 Solution, that's a property of the acid itself, the base itself.

03:42 Solutions can be concentrated or dilute.

03:46 So it's a little bit different.

03:50 So if you look at a beaker here, concentrated just means there's more molecules.

04:02 So let's say these red dots are some molecule.

04:10 Dilute just means there's less of it...

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