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NaOH
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What solution should be used to neutralize spillage of concentrated hcl?
potassium chloride
What happens when HCl is mixed with a solution that is not a buffer solution?
If the solution is not a buffer, the HCl will react with the solution to form a product.
What is the molarity of an hcl solution if 7ml hcl solution is titrated with 27.6ml of 0.170m of naoh solution?
(7 mL)(X M HCl) = (27.6 mL)(0.170 M NaOH)7X = 4.692X = 0.7 M HCl==========
How to prepare 0.2N HCl solution?
0.2 N HCl solution means 0.2 equivalents of HCl dissolved in 1 litre of water. Normality = Molarity x n-factor => Molarity =Normality/n-factor=0.2/1=0.2 M 0.2 moles should be present in 1 litre of solution. 0.2moles =0.2 x 36.5 = 7.3 grams of HCl =>Dissolve 7.3 grams of HCl in 1 litre if water to get a 0.2N solution.
If it requires 40 ml of 3.5 m naoh to neutralize 55 of hcl what is the molarity of the hcl solution?
40 ml of NaOH contains 0.04 L * 3.5 M = 0.14 mole of NaOH Since NaOH donates 1 OH you will also have 0.14 mole of OH- in solution. This can be neutralised with an equal amount of H+. HCl can donate 1 H+, so you need an equal amount of H+ to neutralise the OH-. So you need 0.14 mole of the HCl. 55 ml has 0.14 mole HCl. So the molarity is: 0.14 mole / 0.055 L = 2.54 M
Why was the organic containing HCl was washed with sodium bicarbonate?
To neutralise the acid (HCl).
What solution should be used to neutralize spillage of concentrated hcl?
potassium chloride
What is example of quantitative observation?
Quantitative observations involve numbers. An example would be the volume of 0.1M HCl needed to neutralise 25 ml of sodium hydroxide solution.
What happens when HCl is mixed with a solution that is not a buffer solution?
If the solution is not a buffer, the HCl will react with the solution to form a product.
What is the molarity of an hcl solution if 7ml hcl solution is titrated with 27.6ml of 0.170m of naoh solution?
(7 mL)(X M HCl) = (27.6 mL)(0.170 M NaOH)7X = 4.692X = 0.7 M HCl==========
Is HCL acidic in aqueous solution?
If it is only HCL, yes.
Is methyl orange the indicator used in the titration of na2co3 against hcl solution?
yes it is
How to prepare 0.2N HCl solution?
0.2 N HCl solution means 0.2 equivalents of HCl dissolved in 1 litre of water. Normality = Molarity x n-factor => Molarity =Normality/n-factor=0.2/1=0.2 M 0.2 moles should be present in 1 litre of solution. 0.2moles =0.2 x 36.5 = 7.3 grams of HCl =>Dissolve 7.3 grams of HCl in 1 litre if water to get a 0.2N solution.
If it requires 40 ml of 3.5 m naoh to neutralize 55 of hcl what is the molarity of the hcl solution?
40 ml of NaOH contains 0.04 L * 3.5 M = 0.14 mole of NaOH Since NaOH donates 1 OH you will also have 0.14 mole of OH- in solution. This can be neutralised with an equal amount of H+. HCl can donate 1 H+, so you need an equal amount of H+ to neutralise the OH-. So you need 0.14 mole of the HCl. 55 ml has 0.14 mole HCl. So the molarity is: 0.14 mole / 0.055 L = 2.54 M
What is hydrochloric acid and acid in a aqueous solution?
HCl is ionozed in aq solution HCl + H2O = H3O(+ CHARGE) + Cl (- CHARGE) HCl FORMULA WILL REAMAIN HCl OT WILL BOT CHANGE
Explain why a 0.10 HCL solution is assumed to have a pH value 1?
HCl is a strong acid. Therefore, it can be expected to fully dissociate in aqueous solution, yielding one hydrogen ion and one chloride ion per molecule. The concentration of the hydrogen ion should thus be the same as the initial concentration of the HCl. Therefore, a 0.10M HCl solution has an H+ concentration of 0.10M. By the equation pH=-log[H+], the pH of this solution is 1.
What is the molarity of a solution in which 0.597 moles of HCl are dissolved in 0.169 liters of solution?
Molarity = moles of solute/liters of solution Molarity = 0.597 moles HCl/0.169 liters = 3.53 M HCl ------------------
