# What is the molarity of 4.9\% H2SO4 solution?

Table of Contents

- 1 What is the molarity of 4.9\% H2SO4 solution?
- 2 What is the molarity of H2SO4 solution that has a density 1.84 g CC?
- 3 What is molarity of solution containing 49\% of H2SO4 by mass?
- 4 How do you find the molarity of Sulphuric acid?
- 5 How do you make 0.05 M sulfuric acid?
- 6 What will be the density of 3.6 molar Sulphuric acid having 29 by mass?
- 7 What is the density of an ideal solution of sulfuric acid?
- 8 How many grams of sulfuric acid are in 1 liter of solution?

## What is the molarity of 4.9\% H2SO4 solution?

So molarity is 0.05M.

### What is the molarity of H2SO4 solution that has a density 1.84 g CC?

so molarity = 1 mole / 54.3 ml * 1000 = 18.41 M. Q3. What is the molarity of H2SO4 solution, that has a density 1.84 gm/cc at 35∘C and contains solute 98\% by weight? Q4.

**What is the molarity of 98\% by mass of H2SO4 whose density is 1.8 g mL?**

= 17.98 M. Hence, the molarity of the solution is 17.98 M.

**What is the molarity of H2SO4 solution containing 49\% H2SO4 by mass?**

= 0.590 liter. ⇒ Molarity = 0.75 M. Hence, the Molarity of the solution is 0.75 M.

## What is molarity of solution containing 49\% of H2SO4 by mass?

molarity = 4.09M.

### How do you find the molarity of Sulphuric acid?

1 gram of H2SO4 will be equal to 1/98.08 moles. Therefore, we can say that 1 liter of Sulfuric acid contains 17.822 moles or in other words molarity of 95\% (w/w) Sulfuric acid is equal to 17.822 M….Known values.

Known values | |
---|---|

Molecular weight of H2SO4 | 98.08 g/mole |

Concentration of Sulfuric acid | 95\% (\% by mass, wt/wt) |

**What is the molarity of H2SO4 solution that has a density 1.84 g CC at 35oc and contains 98\% by weight?**

What is the molarity of H2SO4 solution that has a density of 1.84g/cc at 350C and contains 98\% by weight? A . 4.18M.

**What is the molarity of 1 N H2SO4?**

2M

The molarity of 1N SULPHURIC ACID = 2M.

## How do you make 0.05 M sulfuric acid?

- Take 950 ml distilled and cool water in a container.
- Take exactly 2.45 ml( for 0.05 N H2SO4) or 4.9 ml ( for 0.05 M H2SO4 ) pure Sulphuric acid (H2SO4) .
- Now, add Sulphuric acid to the distilled water drop by drop with constant stirring.
- Allow the solution to be cooled.
- Add some more water to make it upto 1000 ml.

### What will be the density of 3.6 molar Sulphuric acid having 29 by mass?

The density (in g mL–1) of a 3.60 M sulphuric acid solution that is 29\% H2SO4 (Molar mass = 98 g mol-) by mass will be. 1.64.

**What is the molarity of 98\% sulfuric acid?**

1.84

Dilutions to Make a 1 Molar Solution

Concentrated Reagents | Density | Molarity (M) |
---|---|---|

Perchloric acid 70\% | 1.67 | 11.6 |

Orthophosphoric acid 85\% | 1.7 | 15.2 |

Sodium hydroxide 47\% | 1.5 | 17.6 |

Sulfuric acid 98\% | 1.84 | 18.4 |

**What is the molarity of a 5\% sulfuric acid solution?**

If it meant exactly 5.00\% w/w, then 0.515M is a good answer. If it meant 5.00\% w/v (5.00 g sulfuric acid in 100 mL solution, then we do not need to multiply times the 1.01 density factor. If they meant 5\% (as in between 4.5\% and 5.4\%) but not exactly 5.00\%, then we can only write 0.5M as the molarity of that solution.

## What is the density of an ideal solution of sulfuric acid?

The expected density for an ideal solution is 1.57 g/mL. Sulfuric acid dissolves in water but not as an ideal solution at higher concentrations. It should take a little less acid to make a 64\% solution. 100 mL solution should weigh 154 grams.

### How many grams of sulfuric acid are in 1 liter of solution?

If the solution concentration is 5\% w/w (5 g of sulfuric acid per 100 g of solution), 1 liter of solution would contain As the molecular weight of sulfuric acid is 98.1, that number of grams of sulfuric acid, translated to moles, is 50.5÷98.1=50.5/98.1=0.515 moles.

**How do you make 75\% acid by volume from 96\% sulfuric acid?**

This is to say that 78.125 mL of 96\% sulfuric acid must be mixed with 21.75 mL of water to prepare 100 mL of a solution that is 75\% acid by volume. You need to clarify the question. You will need a highly concentrated sulfuric acid solution. So you buy some 96\% sulfuric acid, and you have 100 mL of distilled water.