# How many moles sodium bicarbonate are needed to neutralize 0.8ml of sulphuric acid at STP ​

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How many moles sodium bicarbonate are needed to neutralize 0.8ml of sulphuric acid at STP ​

0.0338 moles of sodium bicarbonate are required to react with 0.9 mL 100% sulphuric acid solution Explanation: Equation of the reaction: Na₂CO₃(aq) + H₂SO₄(aq) —> Na₂SO₄(aq) + H₂O(l) + CO₂(g) Since the concentration of the sulphuric acid is not given in the question, the assumption is made that the sulphuric acid solution is 100% sulphuric acid solution. The density of 100% concentrated sulfuric acid is 1.839 g/mL. Amount of acid in 0.9 mL solution = 0.9 mL * 1.839 g/mL = 1.655 g
Number of moles of acid in 1.655 g = mass/molar mass Molar mass of  H₂SO₄ = 98 g/mol Number of moles of acid in 1.471 g = 1.655 g / 98 g/mol = 0.0169 moles From the equation of reaction,  1 mole of H₂SO₄  reacts with 2 moles of Na₂CO₃ 0.0169 moles of H₂SO₄  will react with 0.0169 * 2 moles of Na₂CO₃ = 0.0338 moles Therefore, 0.0338 moles of sodium bicarbonate are required to react with 0.9 mL 100% sulphuric acid solution

8.0356 * 10^-5 moles of NaHCO3 Explanation: Sulphuric acid = H2SO4 Sodium bicarbonate = NaHCO3 The reaction between both compounds is given by; 2NaHCO3(aq) + H2SO4(aq) → Na2SO4(aq) + 2CO2(g) + 2H2O(l) In the reactin above; 2 mol of NaHCO3 neutralizes 1 mol of H2SO4 At stp, 1 mol occupies 22.4 L; 1 mol = 22.4 L = 22400 mL x mol = 0.9 mL x = 0.9 / 22400 = 4.0178 * 10^-5 moles of H2SO4 Since 2 mol = 1 mol from the equation; x mol = 4.0178 * 10^-5 x mol = 2 * 4.0178 * 10^-5 x = 8.0356 * 10^-5 moles of NaHCO3

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n NaHCO3 = 9.6 E-3 mol Explanation: balanced reaction: 2 NaHCO3(s) + H2SO4(ac) ↔ Na2SO4(ac) + 2 CO2(g) + 2 H2O(l)assuming a concentration of H2SO4 6Mnormally worked in the lab ⇒ n H2SO4 = 8 E-4 L * 6 mol/L = 4.8 E-3 mol H2SO4 according to balanced reaction, we have that for every mol of H2SO4 there are two mol of NaHCO3 ( sodium bicarbonate) ⇒ mol NaHCO3 = 4.8 E-3 mol H2SO4 * ( 2 mol NaHCO3 / mol H2SO4 ) ⇒ ,mol NaHCO3 = 9.6 E-3 mol So 9.6 E-3 mol NaHCO3,  are the minimun moles necessary to neutralize the acid.

2 moles of sodium bicarbonate is required for each mole of H2SO4. Originally Answered: How many moles of sodium bicarbonate are needed to neutralise 0.8 ml of sulphuric acid at STP? Explanation:

# How many moles sodium bicarbonate are needed to neutralize 0.8ml of sulphuric acid at STP ​

Looking to neutralize acid in a laboratory setting? Need to know the number of moles of sodium bicarbonate required to achieve the desired pH? This article will provide you with the necessary information needed to achieve the correct result.

## What is sulphuric acid?

Sulphuric acid is a compound made of two molecules of sulphur and one molecule of oxygen. It is a strong acid that is used in many industries, including chemical manufacturing and wine making.

Sulphuric acid can cause serious injury if it is not handled properly. It is important to knows how much sodium bicarbonate is needed to neutralize .ml of sulphuric acid at STP (Standard Temperature and Pressure).

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If .ml of sulphuric acid is mixed with 1 gram of sodium bicarbonate, then the resulting mixture will be neutralized. If .ml of sulphuric acid is mixed with more than 1 gram of Sodium Bicarbonate, then the mixture will become too alkaline and will not react with any more Sulphuric Acid.

## How does sulphuric acid cause injury?

Sulphuric acid is a strong acid that can cause injury if it is ingested or if it is accidentally spilled. It can damage the skin, eyes, and respiratory system. Sulphuric acid is also dangerous because it corrodes metal.

To neutralize sulphuric acid, you need to dissolve it in a liquid. The liquid can be water, but most often it is sodium bicarbonate (baking soda). When you add sodium bicarbonate to sulphuric acid, it transforms into hydrogen gas and sodium chloride (table salt).

The amount of sodium bicarbonate that is needed to neutralize .ml of sulphuric acid at STP (standard temperature and pressure) is 1.414 l.

## How to neutralize sulphuric acid with sodium bicarbonate

Sulphuric acid is a dangerous substance that can cause serious burns if it spills. To avoid this, you need to know how to neutralize it with sodium bicarbonate.

To neutralize sulphuric acid with sodium bicarbonate, you need to combine it with water in an equal amount. Then, pour the mixture into a container and wait until it reaches a pH of 7.0. This will destroy the acid and prevent it from harming your skin or possessions.

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## What are the risks of not doing so?

If you don’t neutralize the sulphuric acid, it will react with the water in the air to form sulphur dioxide and hydrogen gas. This gas is poisonous and can cause problems in your home, office, or restaurant.

Sulphuric acid is used in many industries, including mining, oil and gas extraction, manufacturing, and agriculture. If you don’t neutralize it, it can damage property and injure people.

There are several ways to neutralize sulphuric acid: by adding sodium bicarbonate (baking soda), using an acid-base reaction calculator, or using a water-neutralizing agent. The most effective way is usually through one of these methods.

## Conclusion

There is no definitive answer to this question as it depends on a number of factors, including the specific sulphuric acid and sodium bicarbonate mixture that you are working with and the temperature at which you are performing the reaction. However, in general, it is generally thought that around 1 gram (1 teaspoon) of sodium bicarbonate will neutralize 0.8ml of sulphuric acid.