Determine the volume of 0.145 M NaOH solution required to neutralize each sample of hydrochloric acid. The neutralization reaction is:NaOH(aq)+HCl(aq)→H2O(l)+NaCl(aq)     Part A 20 mL of a 0.145 M HCl solution Express your answer to two significant figures and include the appropriate units.

Consider the following precipitation reaction: 2 K3PO4 (aq) + 3 Co(NO3)2 (aq) → Co3(PO4)2 (s) + 6 KNO3 (aq)   What volume of 0.222 M K3PO4 (aq) in milliliters is needed to react with 36.28 mL of 0.250 M Co(NO3)2 (aq)?

According to the following reaction, what volume (in mL )  of 1.24 M KCl solution is required to react exactly with 50.0 mL of 1.39 M Pb(NO3)2 solution?2 KCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2 KNO3(aq) Write your numerical answer without unit inside the box. The answer should be in three Significant figures and in standard not scientific notation.

In the following reaction, how many milliliters of a 0.194 M copper(II) nitrate solution are needed to completely react with 25.91 mL of a 0.198 M sodium hydroxide solution? Report your answer with 3 significant figures. Cu(NO3)2 (aq) + 2 NaOH (aq) → Cu(OH)2 (s) + 2 NaNO3 (aq) port

A student wants to make a 0.600 M aqueous solution of barium sulfate, BaSO4, and has a bottle containing 12.00 g of barium sulfate. What should be the final volume of the solution?   Find the numerical answer for this question and make sure to include the following: What is the formula for molarity? What is the molar mass for barium sulfate? When you give your numerical answer, what are the correct significant figures and how do you know that is the correct amount?

Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCl(aq), as described by the chemical equation MnO₂ (s) + 4 HCl(aq) →MnCl₂(aq) + 2 H₂O(1) + Cl₂(g) How much MnO₂ (s) should be added to excess HCl(aq) to obtain 295 mL Cl₂(g) at 25 °C and 715 Torr? and X la # mass of MnO₂: 3 E D C $ 4 R F 675 % V T G

Potassium hydrogen phthalate (HKC3H4O4) is a monoprotic acid commonly called KHP. KHP has a molar mass of 204.20 g/mol. A student weighs out 1.345 g of KHP. Titration of this KHP sample required 18.56 mL of NaOH. Calculate the molarity (M) of the base. Enter your answer with the proper significant figures and no units.

What mass of precipitate (in g) is formed when 20.5 mL of 0.500 M Cu(NO₃)₂ reacts with 29.0 mL of 0.500 M NaOH in the following chemical reaction? Cu(NO₃)₂(aq) + 2 NaOH(aq) → Cu(OH)₂(s) + 2 NaNO₃(aq)

A student needs to dilute a 0.36 M Pb(NO3)20.36 M Pb(NO3)2 solution to make 89.089.0 mL of 0.22 M Pb(NO3)20.22 M Pb(NO3)2. Set up the calculation by placing the values with the correct units into the equation. Then, calculate the volume, in milliliters, of the 0.36 M Pb(NO3)20.36 M Pb(NO3)2 solution that is needed.

What mass of precipitate (in g) is formed when 20.5 mL of 0.500 M Cu(NO₃)₂ reacts with 26.0 mL of 0.500 M NaOH in the following chemical reaction? Cu(NO₃)₂(aq) + 2 NaOH(aq) → Cu(OH)₂(s) + 2 NaNO₃(aq)