Table of Contents
- 1 What is the molarity of a 250 mL H2SO4 solution that was made from a 20.0 mL of a 10.0 m stock solution?
- 2 What is the normality of 250 mL?
- 3 What is the molarity of the H2SO4 solution?
- 4 How many millimeters of a 9.0 m H2SO4 solution are needed to make 0.35 L of a 3.5 M solution?
- 5 What is normality of 2 pH H2SO4 solution?
- 6 What will be the normality of aqueous H2SO4 has pH 0?
- 7 What is the concentration of sulfuric acid at P[HX+] = 0?
- 8 What is the equation of normality of a solution?
What is the molarity of a 250 mL H2SO4 solution that was made from a 20.0 mL of a 10.0 m stock solution?
concentration (M) = moles/volume = 0.2/(. 25) = 0.8 M.
What is the normality of 250 mL?
⇒ Normality = 1.1155.52501000=0.08 N.
What is the molarity of the H2SO4 solution?
The molecular weight of H2SO4 is 2+32+64=98. One Liter weighs 1,820 grams. So, the molarity is 1,820/98 = 18 M.
What volume of 0.10 m H2SO4 must be added to 50 mL of a 0.10 M NaOH solution to make a solution in which the molarity of the H2SO4 is 0.050 m?
Answer: The total volume of that must be added is 100 mL.
What is the molarity of an H2SO4 solution if 25.00 mL is exactly neutralized by 32.63 mL of 0.164 M NaOH?
What is the molarity of H2SO4 solution if 25 mL is exactly neutralised with 32.63 mL of 0.164M NaOH? 0.107 M.
How many millimeters of a 9.0 m H2SO4 solution are needed to make 0.35 L of a 3.5 M solution?
You will need 140 mL of 9.0 M H2SO4 to make 350 mL of a 3.5 M solution.
What is normality of 2 pH H2SO4 solution?
For example, a 2 M H2SO4 solution will have a Normality of 4N (2 M x 2 hydrogen ions). A 2 M H3PO4, solution will have a Normality of 6N.
What will be the normality of aqueous H2SO4 has pH 0?
of H+ replaceable ions is 1, hence normality will be 1 N.
How do you calculate H+ ions in a H2SO4 solution?
Normality = Molarity * Valency Factor = 0.1 * 2 =0.2N H2SO4 contributes 2 H+ ions for every mol. Since H2SO4 is a strong acid we can assume 100\% dissociation. Therefore, in a 0.1 M H2SO4 solution we will have 0.2 mol/L of H+ ions. We can express 0.2 as 2 x 10^-1.
What is the pH of a 5m H2SO4?
OK, so it probably is a homework question (the what is the pH of a 5M H2SO4) and yes, using the standard definition for pH (pH = -log [H+]) a diprotic acid, fully dissociated (e.g., H2SO4) at a concentration of 5 M will give 10 M H+ concentration (though perhaps a different activity) and leads to a negative pH (= -1 here).
What is the concentration of sulfuric acid at P[HX+] = 0?
At pH = 0, sulfuric acid is substantially HSOX4X − and HX +, with little HX2SOX4 or SOX4X2 −. Therefore at p[HX +] = 0, sulfuric acid concentration is 1 M, because each mole of sulfuric acid has released one mole of HX +. Normality of an acid is the concentration of the acid times the number of acidic protons per molecule.
What is the equation of normality of a solution?
The equation of normality that helps to estimate the volume of a solution required to prepare a solution of different normality is given by, Initial Normality (N 1 ) × Initial Volume (V 1 ) = Normality of the Final Solution (N 2 ) × Final Volume (V 2 )
https://www.youtube.com/watch?v=3MEnHwtXgqA