Here are the solutions to the naming and formula problems.
Part A: Name the following acids and bases
To solve these, we look at the chemical formula:
*
Bases usually end in
OH. We name the metal first, then add "hydroxide."
*
Acids starting with
H followed by a single element (like Cl or S) start with "Hydro-" and end in "-ic acid."
*
Acids starting with
H followed by a group of elements with Oxygen (like $SO_3$ or $CO_3$) use specific names based on the polyatomic ion (usually ending in "-ic" or "-ous").
*
Special cases: Some common compounds like Ammonia ($NH_3$) have specific common names.
1.
NaOH: Sodium is the metal. OH is hydroxide.
* Answer:
Sodium hydroxide
2.
$H_2SO_3$: This contains the sulfite ion ($SO_3^{2-}$). When turning an "-ite" ion into an acid, it becomes "-ous acid."
* Answer:
Sulfurous acid
3.
$H_2S$: This is Hydrogen + Sulfur. No oxygen means we use "Hydro-" and "-ic."
* Answer:
Hydrosulfuric acid
4.
$NH_3$: This is a very common base known by its common name.
* Answer:
Ammonia
5.
HF: Hydrogen + Fluorine. No oxygen. Use "Hydro-" and "-ic."
* Answer:
Hydrofluoric acid
6.
RbOH: Rb is Rubidium. OH is hydroxide.
* Answer:
Rubidium hydroxide
7.
CsOH: Cs is Cesium. OH is hydroxide.
* Answer:
Cesium hydroxide
8.
HSe: Hydrogen + Selenium. No oxygen. Use "Hydro-" and "-ic."
* Answer:
Hydroselenic acid
9.
HI: Hydrogen + Iodine. No oxygen. Use "Hydro-" and "-ic."
* Answer:
Hydroiodic acid
10.
$H_2CO_3$: This contains the carbonate ion ($CO_3^{2-}$). "-ate" ions become "-ic acids."
* Answer:
Carbonic acid
***
Part B: Write down the formula for the following acids and bases
To solve these, we balance the positive charges (cations) and negative charges (anions) so the total charge is zero.
1.
Potassium hydroxide: Potassium is $K^+$, Hydroxide is $OH^-$. They balance 1-to-1.
* Answer:
KOH
2.
Hydrobromic acid: "Hydro-" means just Hydrogen and Bromine. H is $+1$, Br is $-1$.
* Answer:
HBr
3.
Tin (IV) hydroxide: Tin (IV) means $Sn^{4+}$. Hydroxide is $OH^-$. You need four -1 charges to balance one +4 charge.
* Answer:
$Sn(OH)_4$
4.
Hydrocyanic acid: This is a special acid made of Hydrogen, Carbon, and Nitrogen ($CN^-$).
* Answer:
HCN
5.
Chromic acid: This comes from the chromate ion ($CrO_4^{2-}$). To balance the -2 charge, you need two Hydrogens ($H^+$).
* Answer:
$H_2CrO_4$
6.
Beryllium hydroxide: Beryllium is in Group 2, so it is $Be^{2+}$. Hydroxide is $OH^-$. You need two OH groups.
* Answer:
$Be(OH)_2$
7.
Acetic acid: This is a common organic acid found in vinegar. The formula is standard.
* Answer:
$CH_3COOH$ (or written as $HC_2H_3O_2$)
8.
Strontium hydroxide: Strontium is in Group 2, so it is $Sr^{2+}$. Hydroxide is $OH^-$. You need two OH groups.
* Answer:
$Sr(OH)_2$
9.
Citric acid: This is a common weak acid found in citrus fruits. It has a specific formula.
* Answer:
$C_6H_8O_7$ (often written as $H_3C_6H_5O_7$)
10.
Barium hydroxide: Barium is in Group 2, so it is $Ba^{2+}$. Hydroxide is $OH^-$. You need two OH groups.
* Answer:
$Ba(OH)_2$
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Final Answer:
A. Name the following acids and bases:
1. Sodium hydroxide
2. Sulfurous acid
3. Hydrosulfuric acid
4. Ammonia
5. Hydrofluoric acid
6. Rubidium hydroxide
7. Cesium hydroxide
8. Hydroselenic acid
9. Hydroiodic acid
10. Carbonic acid
B. Write down the formula for the following acids and bases:
1. KOH
2. HBr
3. $Sn(OH)_4$
4. HCN
5. $H_2CrO_4$
6. $Be(OH)_2$
7. $CH_3COOH$
8. $Sr(OH)_2$
9. $C_6H_8O_7$
10. $Ba(OH)_2$
Parent Tip: Review the logic above to help your child master the concept of acid base equations worksheet.
