Since soap and detergent action is hindered by hard water, laundry formulations usually include water softeners—called builders—designed to remove hard water ions (especially Ca2+ and Mg2+from the water. A common builder used in North America is sodium carbonate. Suppose that the hard water used to do laundry contains 75 ppm CaCO3   and 55 ppm MgCO3 (by mass). What mass of Na2CO3 will remove 90.0% of these ions from 10.0 L of laundry water?

I just need the mechanism for the reaction. THe starting product is 1,7-dimethyl-heptanedioate, with the reagent NaOMe, and solvent ether.

You have 1.5 liter of solution that is composed of 8.88 grams of NH3 and 11.33 grams of ammonium chloride mixed well. Kb for ammonia =1.8 x 10^-5 (A) is this a buffer solution? Why or why not? (B)if it is a buffer solution, what is the pH of this buffer solution? (C)how many mL of 1.50 M HCl can be added to this solution before the buffer is exhausted (d) how many mL of 1.5 M NaOH can be added to this solution before the buffer is exhausted?

Calculate the concentration (molarity) of Pb2+ ions in a solution made by adding 0.010 moles of Pb(NO3)2 to 1.0 L of a  2.0 M NaI solution.  (Kf = 3.0 x 104 for PbI42−) - 4.9 x 10−2 -3.3 x 10−5 - 2.1 x 10−7 -1.7 x 10−7 -2.3 x 10−8

do both please as they are the part of the same question..

18.57grams of Ce(NO3)4 are required to make the solution. (I don't know if you need that information to solve this question but that is the answer to question a)

Determine the compound that is expected to be more soluble in acidic solution than in neutral or basic solution. О KBr O BaCl2 O Ni(OH)2 O Cu(NO3)2

1. How do you prepare a 100mL of 0.1 M phosphate buffer?To make 100 mL of 0.1 M phosphate buffer: Calculate the amount of sodium phosphate needed. moles of sodium phosphate = (0.1 mol/L) x (0.1 L) = 0.01 moles mass of sodium phosphate = moles x molar mass = 0.01 moles x 142 g/mol = 1.42 g Dissolve 1.42 g of sodium phosphate in distilled water in a 100 mL volumetric flask. Adjust the pH of the solution to the desired value (usually around 7.4) using a strong acid or strong base. Bring the solution to the final volume (100 mL) with distilled water.   2. From the anterior buffer, how do you make 100mL of 0.05 M? To make 100 mL of 0.05 M phosphate buffer from the 0.1 M stock solution: Calculate the amount of the 0.1 M phosphate buffer needed. moles of phosphate buffer = (0.05 mol/L) x (0.1 L) = 0.005 moles Calculate the volume of the 0.1 M phosphate buffer needed. moles = concentration x volume (in liters) volume = moles / concentration = 0.005 moles / 0.1 mol/L = 0.05 L or 50 mL Measure…

2. The overall reaction in a commercial heat pack can be represent 4Fe(s) + 30₂ (g) 2Fe₂O3 (8) How much heat is released when 1.00 mole of Fe₂O3 is produced? a)-1652 kJ b) + 1652 kJ e) - 826 kJ d) + 826 kJ ΔΗ = - 1652 kJ

Buffer capacity is a measure of a buffer solution's resistance to changes in pH as strong acid or base is added. Suppose that you have 105 mL of a buffer that is 0.260 M in both benzoic acid (CH₂COOH) and its conjugate base (CH₂COO¯). Calculate the maximum volume of 0.270M HCl that can be added to the buffer before its buffering capacity is lost. volume: mL