Question

In: Chemistry

4. 62.4 mL of 0.39 M NaCl solution was added to 26.8 mL of 058 M...

4. 62.4 mL of 0.39 M NaCl solution was added to 26.8 mL of 058 M Pb(NO3)2 solution. a. Write the full balanced reaction, the molecular ionic equation and the net ionic equation.
b. What is the precipitate? c. How many grams of the precipitate can be made

Solutions

Expert Solution


Related Solutions

You have 420 mL of an aqueous solution that is 0.39 M Na2SO4 and a separate...
You have 420 mL of an aqueous solution that is 0.39 M Na2SO4 and a separate 185 mL aqueous solution that is 0.45 M BaCl2. a). How many moles of each of the four ions are present ? Na+ SO42- Ba2+ Cl- b). When these two solutions are mixed together, what is the chemical formula of the solid expected to precipitate from the mixture? c). If the sulfate ions in the mixed solution react with the barium ions in the...
(a) 3.25 M NaCl solution (density of solution = 1.08 g/mL)
  Calculate the molality of each of the following aqueous solutions.   (a) 3.25 M NaCl solution (density of solution = 1.08 g/mL) m   (b) 51.4 percent by mass KBr solution m  
You mixed 600 mL of 5M NaCl and 150 mL of sodium citrate solution and added...
You mixed 600 mL of 5M NaCl and 150 mL of sodium citrate solution and added 250 mL of water to make a 1L stock 20X SSC (standard sodium citrate) buffer. With 40 grams of SDS, sodium dodecyl sulfate you made 800 mL of a 5% SDS solution. ~Calculate how much SDS and SSC you need from the above solutions to make 1 Liter of 0.1X SSC, 0.1% SDS.
A solution prepared by mixing 22.4 mL of 0.380 M NaCl and 22.4 mL of 0.380...
A solution prepared by mixing 22.4 mL of 0.380 M NaCl and 22.4 mL of 0.380 M KI was titrated with 0.190 M AgNO3 in a cell containing a silver indicator electrode and a saturated calomel reference electrode. (a) What is [Ag ] when 21.2 mL of 0.190 M AgNO3 have been added? Express your answer as x, where [Ag ] is a quotient having the form Ksp,AgI/x. (b) What is [Ag ] when 67.0 mL of 0.190 M AgNO3...
If 100.mL of 0.035 M HCl solution is added to 220.mL of a buffer solution which...
If 100.mL of 0.035 M HCl solution is added to 220.mL of a buffer solution which is 0.20M in NH3 and 0.18M in NH4Cl, what will be the pH of the new solution? The Kb of NH3 is 1.8x10^-5. Please explain how the answer was obtained. Thank you!
When 10.0 mL of 1.00 M AgNO3 solution is added to 10.0 mL of 1.00 M...
When 10.0 mL of 1.00 M AgNO3 solution is added to 10.0 mL of 1.00 M NaCl solution at 25.0 ° C in a calorimeter, a white precipitate of AgCl forms and the temperature of the aqueous mixture increases to 32.6 ° C. Assuming that the specific heat of the aqueous mixture is 4.18 J/(g °C), the density of the mixture is 1.00 g/mL, and the calorimeter itself absorbs a negligible amount of heat, what is ΔH in kJ/mol AgCl...
11 mL of 0.0100 M HCl are added to 25.0 mL of a buffer solution that...
11 mL of 0.0100 M HCl are added to 25.0 mL of a buffer solution that is 0.010 M HC2H3O2 and 0.08 M C2H3O2-.  What is the pH of the resulting solution?
A membrane separates two solutions. Solution C is 300 mL of 0.2 M NaCl, and Solution...
A membrane separates two solutions. Solution C is 300 mL of 0.2 M NaCl, and Solution D is 500 mL of 0.6 M NaCl. The membrane is permeable to water, sodium ions, and chloride ions. After 24 hours, what will be the chloride ion concentration in Solution C? Show your calculations.
When 220 mL of 1.50x10^-4 M hydrochloric acid is added to 135 mL of 1.75x10^-4 M...
When 220 mL of 1.50x10^-4 M hydrochloric acid is added to 135 mL of 1.75x10^-4 M Mg(OH)2, the resulting solution will be
A student added 50.0 mL of an NaOH solution to 100.0 mL of 0.300 M HCl....
A student added 50.0 mL of an NaOH solution to 100.0 mL of 0.300 M HCl. The solution was then treated with an excess of aqueous chromium(III) nitrate, resulting in formation of 2.36 g of precipitate. Determine the concentration of the solution.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT