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If 0.235 g of KHP requires 16.73 mL of NaOH solution to nuetralize it, calculate the molarity of the NaOH solution
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- If 0.235 g of KHP (potassium hydrogen phthalate) require 15.5 mL of NaOH solution to neutralize it, calculate the molarity of the NaOH solution.300 milliliters of a stock solution of potash of alum was mixed with sterile normal saline to prepare 3 liters of 1% alum irrigation. Calculate the percent strength of the stock solution. An alkaline stock solution was prepared by dissolving 50 grams of sodium carbonate in purified water USP to prepare 1 liter solution. How many milliliters of 2.5% sodium carbonate can be prepared from the stock solution?Calculate the volume in liters of 0.5-N solution that can be prepared from 20g of phosphoric acid (H3PO4).
- What is the molarity of a solution in which 150.0 grams of iodine, I2I2, are dissolved in rubbing alcohol for a final volume of 500.0 mL?The number of moles of H2O produced in reaction of 50 mL 1.0 M HCl and 50 mL 1.0 M NaOH: (5.00×10−2) Joules released per mole of water formed: ?how many grams of phosphoric acid (H3PO4) are needed to prepare 25.0 m of an acid solution that is 0.20 N in reactions where the three hydrogen ions replaced?
- A solution of H2SO4 is found to be 0.5172 N and 39.65 mL of it are equivalent to 21.74 mL of standard alkali solution. What is the N of the alkali and how many grams of sulfamic acid (HSO3.NH2) will 1.oo mL of it neutralize?Calculate the concentration of nitrate ion in a solution of 0.10M barium nitrate solution following the epectroneutrality principle (ENP).How many grams of (NH4)2SO4 should be present to prevent precipitation of Mg(OH)2(s)?
- By analogy to examples given in the text, predict what gas forms when Na2SO3(s)reacts with HCl(aq).What mass of Hydrazine reacts with 250mL of 0.146M H2SO41. Calculate the molarity of a solution prepared by dissolving 11.5 g of solid NaOH in enogh water to make 1.50 L solution. 2. Give the concentration of each type of ion in the following solutions: a) 0.50 M Co(NO3)2 b) 1 M Fe(ClO4)3