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You are asked to prepare a pH = 4.0 buffer starting from 1.50 L of 0.0200M solution of benzoic acid (C6H5COOH) and an excess of sodium benzoate (C6H5COONa) .
What is the pH of the benzoic acid solution prior to adding sodium benzoate?
How many grams of sodium benzoate should be added to prepare the buffer? Neglect the small volume change that occurs when the sodium benzoate is added
Determine the empirical formula of a compound that is 32.79% Na,12.90% Al with the remainder F.If the molecular mass is approximately 200 amu
How many moles of CO2 will be produced if 3.119 g of O2 are reacted completely?
Sucrose and glucose are nonvolatile. What is the mole fraction of water in this solution?
the reduction table in your notes, calculate the standard cell potential for the following reaction. F2(g) + 2 Cl-(aq) 2 F-(aq) + Cl2(g)
A saturated solution of calcium hydroxide contains .38 grams of calcium hydroxide in each 250 mL of solution. What is the pH of the saturated calcium hydroxide?
Copper metal reacts with hot concentrated sulfuric acid solution to form aqueous copper (II) sulfate, sulfur dioxide gas, and water. Write the balanced chemical formula.
A 10 ml sample of gastric juice was obtained from a patient several hours after a meal. The gastric juice was then titrated with 7.2 ml of 0.1 M NaOH to neutrality
Help me understand specifically why the dissociated phosphate ion would prefer to bond with cations like Al and Zn. I think I know why but help me better understand.
The pressure is changed to 8.75 atm and the gas is cooled to 15 C. Calculate the new volume of the gas using the ideal gas equation.
30.0 mL of a 3.0 M KOH solution are diluted to 250.0 mL. What is the molarity of the diluted KOH solution? 3)what volume of 1.00 M NaOH is required to prepare 500.0 mL of 0.250 M NaOH? then explain how to prepare this solution.
1.248-g sample of limestone rock is pulverized and then treated with 30.00 mL of 1.035 M HCl solution. the excess acid then requires 11.56 mL of 1.010 M NaOH for neutralization.
Concentrated stock HCl has a molecular weight of 36.46 and contains 32g of salt for every 100g of acid (termed as 32% w/w). To prepare molar solutions %w/w must be converted into %w/v by considering the density of stock HCl which is 1.16.
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