An exchange reaction is carried out using a solution of aqueous lead (II) nitrate. A precipitate is formed by adding a solution containing excess sodium hydroxide. The mass of the precipitate was found to be 1.1 grams. What was the concentration of the original lead nitrate solution if its original volume was 45 mL? 2NAOH(aq)+Pb(NO,),(aq)→Pb(OH),(s)+2NANO,{aq) • Previous Next Not saved Subr

Consider the reaction: Ag⁺(aq) + Cl⁻(aq) → AgCl(s) How many grams of NaCl would be needed to precipitate the Ag⁺ ions from 2.650 × 10² mL of a 0.0115 M AgNO₃ solution? The molar mass of NaCl is 58.44 g/mol.

If 28.5 g of NaOH is added to 0.800 L of 1.00 M Zn(NO₃)₂, what mass in grams of Zn(OH)₂ will be formed in the following precipitation reaction? 2 NaOH(aq) + Zn(NO₃)₂(aq) → Zn(OH)₂ (s) + 2 NaNO₃ (aq)

Consider the reaction: Ag⁺(aq) + Cl⁻(aq) → AgCl(s) How many grams of NaCl would be needed to precipitate the Ag⁺ ions from 2.600 × 10² mL of a 0.0115 M AgNO₃ solution? The molar mass of NaCl is 58.44 g/mol.

A sample of 1.975 g oxalic acid dehydrate (H2C2O4 . 2H2O) was dissolved in enough water to make a 250.0 mL solution. What is the concentration of oxalic acid in the solution?In solid form, the dihydrate crystal lattice contains two water molecules for every oxalic acid molecule. The water molecules must be included as part of the molar mass. The molar mass of H2C2O4 * 2H2O is 126.064 g/mol. Oxalic acid is a diprotic acid (H2A). Write the balanced reaction for aqueous oxalic acid reacting with aqueous potassium hydroxide. If 20.00 mL of the oxalic acid solution described above is placed in a flask and then titrated with 0.1525 M potassium hydroxide, what volume of the potassium hydroxide solution would be required for a complete reaction?

If 32.5 g of NaOH is added to 0.550 L of 1.00 M Ni(NO₃)₂, how many grams of Ni(OH)₂ will be formed in the following precipitation reaction? 2 NaOH(aq) + Ni(NO₃)₂(aq) → Ni(OH)₂ (s) + 2 NaNO₃ (aq)

If 16.5 g of NaOH is added to 0.550 L of 1.00 M Ni(NO₃)₂, how many grams of Ni(OH)₂ will be formed in the following precipitation reaction?2 NaOH(aq) + Ni(NO₃)₂(aq) → Ni(OH)₂ (s) + 2 NaNO₃ (aq)

What quantity in moles of precipitate will be formed when 100.0 mL of 2.00 M NaI is reacted with 80.0 mL of 0.900 M Pb(NO₃)₂ in the following chemical reaction?2 NaI(aq) + Pb(NO₃)₂(aq) → PbI₂(s) + 2 NaNO₃(aq)

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?