Table of Contents

## How do you figure formula mass?

Explanation: To calculate formula mass, multiply the subscript of each element in the formula by the element’s atomic weight (relative atomic mass) found on the periodic table. The unit for formula mass is either u or Da (Daltons).

**What is the molar mass of hydrate?**

8.1 Molar mass

Hydrate type | Molar mass (g/mol)a | |
---|---|---|

Isobutane | II | 20.24 |

CO2 | I | 21.59 |

H2S | I | 20.87 |

### What is the formula for calculating?

For simple formulas, simply type the equal sign followed by the numeric values that you want to calculate and the math operators that you want to use — the plus sign (+) to add, the minus sign (-) to subtract, the asterisk (*) to multiply, and the forward slash (/) to divide.

**What is a hydrate formula?**

Formula of a Hydrate (Anhydrous Solid⋅xH2O) In order to determine the formula of the hydrate, [Anhydrous Solid⋅xH2O], the number of moles of water per mole of anhydrous solid (x) will be calculated by dividing the number of moles of water by the number of moles of the anhydrous solid (Equation 2.12. 6).

#### What is the formula mass of cuso4?

159.609 g/mol

Copper(II) sulfate/Molar mass

**What is the formula for calculating percentage with example?**

1. How to calculate percentage of a number. Use the percentage formula: P% * X = Y

- Convert the problem to an equation using the percentage formula: P% * X = Y.
- P is 10%, X is 150, so the equation is 10% * 150 = Y.
- Convert 10% to a decimal by removing the percent sign and dividing by 100: 10/100 = 0.10.

## How do you determine the formula of a hydrate?

Formula of a Hydrate (\\(\ext{ Anhydrous Solid}\\ce{*}x\\ce{H2O}\\)) The formula of a hydrate can be determined by dehydrating a known mass of the hydrate, then comparing the masses of the original hydrate and the resulting anhydrous solid.

**What was the mass of the hydrate sample?**

See the answer. The mass of a hydrate was found to be 2.7090 grams. After heating, the anhydrous sample had a mass of 1.8820 grams.

### What is the empirical formula of the hydrate?

Empirical Formula of the Hydrate. Copper (II) Sulfate: Anhydrous Salt: 7.2g(1.00 mole /159.607g) = 0.045 mole. Water: 3.8g(1.00 mole / 18.014g) = 0.21 mole. CuSO4 = 0.045 mole / 0.045 mole = 1 ( * 3) = 3. H2O = 0.21 mole / 0.045 mole = 4.6666666667 ( * 3) = 14.

**What is the formula for the hydrate?**

Determining the Formula of a Hydrate Calculate the gram formula mass of the salt and the water separately. Hint: It is helpful to remember that the gram formula mass of water is 18.0 grams/mole. Divide each given mass or percentage by the substance’s gram formula mass. CaSO 3: 76.9÷ 120.2 = 0.640 H 2 O: 23.1÷ 18.0 = 1.28 Divide each result by the smallest result. the Formula of a Hydrate&chap=7