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The normality is o,3.
12.97
The normality of a solution is the gram equivalent weight of a solute per liter of solution. For example, 1 M sulfuric acid (H2SO4) is 2 N for acid-base reactions because each mole of sulfuric acid provides 2 moles H+ ions.
Calculus with (units) in brackets shows the way how and why.275 (g) / 97.9 (g/mol) = 2.81 mol in 120 L = 2.81 (mol) / 120 (L) = 2.34*10-2 (mol/L) = 0.0234 M H3PO4And since there are 3 protons available per mole: 0.0234 (M) H3PO4 * 3(N/M) = 0.0702 N
3 moles in 1 liter = 3 M
The normality is o,3.
Will not Precipitate
0.08 n
http://wiki.answers.com/Q/Calculate_for_a_solution_formed_by_adding_4.80ml_of_0.130_M_KOH_to_19.0ml_of_7.6x102_M_of_CaOH2"
12.97
The normality of a solution is the gram equivalent weight of a solute per liter of solution. For example, 1 M sulfuric acid (H2SO4) is 2 N for acid-base reactions because each mole of sulfuric acid provides 2 moles H+ ions.
The concentration of the OH- is 8.0 x 10-4 In terms of molarity, since the hydroxide is double that of the calcium, double the molarity of the solution.
Molarity = moles of solute/Liters of solution Molarity = 6 Moles NaCl/2 Liters = 3 M NaCl ========
Normality is the number of gram equivalents of solute per liter of solution.N = [ ( m ) / ( M ) ( Z ) ] [ 1000 / V in mL ]where Z represents the number of H+ ions that the one molecule of the solute is capableof releasing or reacting with. For HCl, Z = 1 .N = [ ( 3.65 g ) / ( 36.458 g / mol ) ( 1 ) ] [ 1000 mL / 1000 mL )N = 0.100 N
Calculus with (units) in brackets shows the way how and why.275 (g) / 97.9 (g/mol) = 2.81 mol in 120 L = 2.81 (mol) / 120 (L) = 2.34*10-2 (mol/L) = 0.0234 M H3PO4And since there are 3 protons available per mole: 0.0234 (M) H3PO4 * 3(N/M) = 0.0702 N
Sulfuric acid H2SO4 will give away 2 protons H+ for this reason its normality is 2 times its molarity. so for H2SO4 M = 2N For HCl M= 1N because HCl has only one proton H+ H3PO4 for example has 3N = M so for your case, 6M = 2N and N= 6/2 = 3.
The normality of commercial grade hydrochloric acid (HCl) can vary depending on the concentration specified by the manufacturer. Hydrochloric acid is commonly available in different concentrations, such as 37% or concentrated hydrochloric acid. To determine the normality, it is essential to know the molarity (moles of solute per liter of solution) and the number of equivalents of the acid. Normality (N) is related to molarity (M) by the equation: � = � × � N=n×M where: � N is the normality, � n is the number of equivalents, � M is the molarity. For hydrochloric acid (HCl), which is a monoprotic acid (donates one proton), the number of equivalents ( � n) is equal to 1. Therefore, if you know the molarity of the commercial grade hydrochloric acid, you can determine its normality using the equation mentioned above. It's important to check the product label or contact the manufacturer for the specific concentration of the hydrochloric acid you are using.