What is the concentration (in molarity) of the Na+ ions in 0.200 L of 0.525 M Na2SO4 (aq)

How many milliliters of 10.0 M HCl(aq) are needed to prepare 920.0 mL of 1.00 M HCl(aq)?

What volume of 0.200 M HNO3(aq) is required to react completely with 0.0150 moles of NaOH?

How many grams of Ag₂CO3 will precipitate when excess Na₂CO3 solution is added to 49.0 mL of 0.590 M AgNO3 solution? 2AgNO3(aq) + Na2CO3(aq) → Ag2 CO3(s) + 2NaNO3(aq) g

A 3.27 g sample of iron ore is transformed to a solution of iron(II) sulfate, FeSO4. This solution is titrated with 0.110 M K2CT20, (potassium dichromate). If it requires 58.3 ml of potassium dichromate solution to titrate the iron(II) sulfate solution, what is the percentage of iron in the ore? The reaction is 6FESO, (aq) + K, Cr2O; (aq) + 7H;SO4 (aq) + 3Fe; (SO,)a (aq) + Cr2 (SO4)a (ag) + 7H2O(1) + K2SO, (ag) Percentage =

In the neutralization of aqueous acetic acid with aqueous calcium hydroxide, 55.7 mL of 0.100 M Ca(OH)2 was required to react with 15.0 mL of CH3COOH.  What was the molarity of the acetic acid solution?

What mass (g) of NaOH is required to make 262 ml of 0.41 M NaOH(aq) solution?

Calculate the number of milliliters of 0.689 M NaOH required to precipitate all of the A1³+ ions in 163 mL of 0.784 M Al2(SO4)3 solution as Al(OH)3. The equation for the reaction is: Al2(SO4)3 (aq) + 6NaOH(aq) → 2Al(OH)3 (s) + 3Na2SO4 (aq) Volume = | mL

What mass of Mg, in g, is required to react with 63.4 mL of 0.269 M AgNO3 solution? Mg(s) + 2AgNO3(aq) → 2Ag(s) + Mg(NO3)2(aq) g Mg

In the neutralization of aqueous acetic acid with aqueous calcium hydroxide, 55.7 mL of 0.100 M Ca(OH)2 was required to react with 15.0 mL of CH3COOH.  What was the molarity of the acetic acid solution?