QuestionWhat is the conjugate acid of $\mathrm{HPO}_{3}{ }^{2-}$ ? Express your answer as a chemical formula. View Available Hint(s) $\square$ Aг $\phi$ $x^{a}$ $x_{b}$ a $\frac{a}{b}$ $\bar{x}$ $\rightarrow$ $\rightleftharpoons$ - (x) A chemical reaction does not occur for this question.

Studdy Solution

STEP 1

What is this asking? We need to figure out what the conjugate acid of $\mathrm{HPO}_{3}{ }^{2-}$ is! Watch out! Don't accidentally find the conjugate base!
We're looking for the acid!

STEP 2

1. Define conjugate acids and bases
2. Find the conjugate acid

STEP 3

A Brønsted-Lowry acid is a proton ( $\mathrm{H}^{+}$ ) donor, and a Brønsted-Lowry base is a proton ( $\mathrm{H}^{+}$ ) acceptor.
When an acid donates a proton, it becomes its conjugate base.
When a base accepts a proton, it becomes its conjugate acid.
They're like two sides of the same coin!

STEP 4

Think of it like this: If we have hydrochloric acid, $\mathrm{HCl}$ , it can donate a proton to become the chloride ion, $\mathrm{Cl}^{-}$ . $\mathrm{HCl}$ is the acid, and $\mathrm{Cl}^{-}$ is its conjugate base.
They're a pair!

STEP 5

Our starting material, $\mathrm{HPO}_{3}{ }^{2-}$ , is acting as a base.
That means it's going to accept a proton!

STEP 6

When $\mathrm{HPO}_{3}{ }^{2-}$ accepts a proton ( $\mathrm{H}^{+}$ ), it gains an $\mathrm{H}$ and becomes $\mathrm{H}_{2} \mathrm{PO}_{3}{ }^{-}$ .
Notice the charge also becomes more positive, going from -2 to -1, because we added a positive charge!

STEP 7

So, the conjugate acid of $\mathrm{HPO}_{3}{ }^{2-}$ is $\mathrm{H}_{2} \mathrm{PO}_{3}{ }^{-}$ !

STEP 8

$\mathrm{H}_{2} \mathrm{PO}_{3}{ }^{-}$

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QuestionWhat is the conjugate acid of $\mathrm{HPO}_{3}{ }^{2-}$ ? Express your answer as a chemical formula. View Available Hint(s) $\square$ Aг $\phi$ $x^{a}$ $x_{b}$ a $\frac{a}{b}$ $\bar{x}$ $\rightarrow$ $\rightleftharpoons$ - (x) A chemical reaction does not occur for this question.

Studdy Solution

STEP 1

What is this asking? We need to figure out what the conjugate acid of $\mathrm{HPO}_{3}{ }^{2-}$ is! Watch out! Don't accidentally find the conjugate base!
We're looking for the acid!

STEP 2

1. Define conjugate acids and bases
2. Find the conjugate acid

STEP 3

A Brønsted-Lowry acid is a proton ( $\mathrm{H}^{+}$ ) donor, and a Brønsted-Lowry base is a proton ( $\mathrm{H}^{+}$ ) acceptor.
When an acid donates a proton, it becomes its conjugate base.
When a base accepts a proton, it becomes its conjugate acid.
They're like two sides of the same coin!

STEP 4

Think of it like this: If we have hydrochloric acid, $\mathrm{HCl}$ , it can donate a proton to become the chloride ion, $\mathrm{Cl}^{-}$ . $\mathrm{HCl}$ is the acid, and $\mathrm{Cl}^{-}$ is its conjugate base.
They're a pair!

STEP 5

Our starting material, $\mathrm{HPO}_{3}{ }^{2-}$ , is acting as a base.
That means it's going to accept a proton!

STEP 6

When $\mathrm{HPO}_{3}{ }^{2-}$ accepts a proton ( $\mathrm{H}^{+}$ ), it gains an $\mathrm{H}$ and becomes $\mathrm{H}_{2} \mathrm{PO}_{3}{ }^{-}$ .
Notice the charge also becomes more positive, going from -2 to -1, because we added a positive charge!

STEP 7

So, the conjugate acid of $\mathrm{HPO}_{3}{ }^{2-}$ is $\mathrm{H}_{2} \mathrm{PO}_{3}{ }^{-}$ !

STEP 8

$\mathrm{H}_{2} \mathrm{PO}_{3}{ }^{-}$

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Studdy Solution

STEP 1

What is this asking? We need to figure out what the conjugate *acid* of HPO32− \mathrm{HPO}_{3}{ }^{2-} HPO3​2− is! Watch out! Don't accidentally find the conjugate *base*!We're looking for the *acid*!

STEP 2

1. Define conjugate acids and bases2. Find the conjugate acid

STEP 3

STEP 4

Think of it like this: If we have hydrochloric acid, HCl \mathrm{HCl} HCl, it can donate a proton to become the chloride ion, Cl− \mathrm{Cl}^{-} Cl−. HCl \mathrm{HCl} HCl is the acid, and Cl− \mathrm{Cl}^{-} Cl− is its conjugate base.They're a pair!

STEP 5

Our starting material, HPO32− \mathrm{HPO}_{3}{ }^{2-} HPO3​2−, is acting as a base.That means it's going to *accept* a proton!

STEP 6

STEP 7

So, the conjugate acid of HPO32− \mathrm{HPO}_{3}{ }^{2-} HPO3​2− is H2PO3− \mathrm{H}_{2} \mathrm{PO}_{3}{ }^{-} H2​PO3​−!

STEP 8

H2PO3− \mathrm{H}_{2} \mathrm{PO}_{3}{ }^{-} H2​PO3​−

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What is this asking? We need to figure out what the conjugate acid of $\mathrm{HPO}_{3}{ }^{2-}$ is! Watch out! Don't accidentally find the conjugate base!
We're looking for the acid!

1. Define conjugate acids and bases
2. Find the conjugate acid

Think of it like this: If we have hydrochloric acid, $\mathrm{HCl}$ , it can donate a proton to become the chloride ion, $\mathrm{Cl}^{-}$ . $\mathrm{HCl}$ is the acid, and $\mathrm{Cl}^{-}$ is its conjugate base.
They're a pair!

Our starting material, $\mathrm{HPO}_{3}{ }^{2-}$ , is acting as a base.
That means it's going to accept a proton!

So, the conjugate acid of $\mathrm{HPO}_{3}{ }^{2-}$ is $\mathrm{H}_{2} \mathrm{PO}_{3}{ }^{-}$ !

$\mathrm{H}_{2} \mathrm{PO}_{3}{ }^{-}$