Calculate the mass of MgCO3 precipitated by mixing 10.00 mL of a 0.200 M Na2CO3 solution with 5.00 mL of a 0.0700 M Mg(NO3)2 solution.
Calculate the mass of MgCO3 precipitated by mixing 10.00 mL of a 0.200 M Na2CO3 solution...
Calculate the mass of MgCO3 precipitated by mixing 10.00 mL of a 0.200 M Na2CO3 solution with 5.00 mL of a 0.0550 M Mg(NO3)2solution.
Calculate the mass of MgCO3 precipitated by mixing 10.00 mL of a 0.200 M Na2CO3 solution with 5.00 mL of a 0.0550 M Mg(NO3)2solution.
What mass of magnesium carbonate is precipitated by mixing 10.0 mL of a 0.200 M sodium carbonate solution with 5.00 mL of a 0.0500 M magnesium nitrate solution?
a) Calculate the pH of the resulting solution obtained by adding 10.00 mL of 0.200 M HCl (strong acid) to 7.50 mL of 0.100 M NaOH (strong base). b) Calculate the pH of the resulting solution obtained by adding 10.00 mL of 0.200 M CH3CO2H (weak acid) to 7.50 mL of 0.100 M NaOH (strong base).
Question 1. A student was given 10.00 mL of a solution of a 0.1162M Na2CO3 solution. What mass (in g) of Na2CO3 is in that 10.00 mL? Question 2. What volume of 0.1527 M HCl (in mL) will it take to titrate the sample in question 1 to the final endpoint?
Calculate the pH of the resulting solution obtained by adding 10.00 mL of 0.200 M HCl (strong acid) to 7.50 mL of 0.100 M NaOH (strong base).
Calculate the pH of the resulting solution obtained by adding 10.00 mL of 0.200 M CH3CO2H (weak acid) to 7.50 mL of 0.100 M NaOH (strong base).
Consider the mixing of 200.0 mL of 0.200 M lanthanum nitrate, La(NO3 )3 , with 400.0 mL of 0.400 M potassium iodate, KIO3 . Calculate the concentration of each of the following ions in the solution: La3+, NO3 –, K+, and IO3 - .
A solution is prepared by mixing 47.00 mL of 0.024 M AgNO3 with 11.00 mL of 1.0×10-3M Na2CO3. Assume that volumes are additive. Calculate [Ag+], [CO32–], [Na+], and [NO3–] after equilibrium is established. [Ag+]= [CO32+]= [Na+]= [NO3-]=
3) Calculate the pH of a solution by mixing 50.0 mL of 0.200 M Na2HPO4 with 20.0 mL 0.0400 M NaH2PO4. (Hint: Buffer solution. Use Henderson-Hasselbalch equation) H3PO4 5 H+ + H2PO4 pkı = 2.1 H2PO4 5 H+ + HPO42- pK2 = 7.2 HPO42- 5 H+ PO43- pK3 = 12.3