A volume of 37.2 mL of a 3.16 M KMnO4 solution is mixed with 15.7 mL of a 0.192 M KMnO4 solution. Calculate the concentration of the final solution. Please answer with correct rounding of numbers.
A volume of 37.2 mL of a 3.16 M KMnO4 solution is mixed with 15.7 mL...
A volume of 36.2 mL of a 0.268 M Ca(NO3)2 solution is mixed with 90.5 mL of a 1.196 M Ca(NO3)2 solution. Calculate the concentration of the final solution.
A)A volume of 46.2 mL of a 0.568 M Ca(NO3)2 solution is mixed with 75.5 mL of a 1.496 M Ca(NO3)2 solution. Calculate the concentration of the final solution. Calculate the molarity of each of the following solutions. (b) 7.25 g of methanol (CH3OH) in × 102 mL of solution: mol/L (c) 9.68 g of calcium chloride (CaCl2) in 2.20 × 102 mL of solution: mol/L (d) 8.57 g of naphthalene (C10H8) in 85.2 mL of benzene solution: mol/L
A solution of 0.200 M KOH (17.6 mL) is mixed with 45.9 mL of 0.143 M HCl. Assuming that the final volume is the sum of the initial volumes, calculate: (a) the molarity of the K+ cation (b) the molarity of the Cl- anion (c) the pH of the final solution (d) the pOH of the final solution
A 185.0 mL solution of 2.714 M strontium nitrate is mixed with 215.0 mL of a 3.460 M sodium fluoride solution. Calculate the mass of the resulting strontium fluoride precipitate. mass: g Assuming complete precipitation, calculate the final concentration of each ion. If the ion is no longer in solution, enter a 0 for the concentration. [Na+]= M [NO−3]= M [Sr2+]= M [F−]= M
A 150.0 mL solution of 3.241 M strontium nitrate is mixed with 205.0 mL of a 3.569 M sodium fluoride solution. Calculate the mass of the resulting strontium fluoride precipitate. mass: g Assuming complete precipitation, calculate the final concentration of each ion. If the ion is no longer in solution, enter a 0 for the concentration. [Na+]= M [NO−3]= M [Sr2+]= M [F−]=
A 165.0 mL solution of 2.777 M strontium nitrate is mixed with 210.0 mL of a 3.278 M sodium fluoride solution. Calculate the mass of the resulting strontium fluoride precipitate Number Assuming complete precipitation, calculate the final concentration of each ion. If the ion is no longer in solution, enter a zero for the concentration. Number Number 2+ Na Number Number
167 mL of 4.7 M HBr solution is mixed with 176 mL of NaOH solution of unknown concentration. The H+ concentration in the final solution is 0.09M. What was the NaOH concentration of the unknown solution?
If 5.25 mL of a 0.278 M solution of NaOH is required to neutralize 15.7 mL of a HCl solution, What is the concentration of the HCl solution? Select one: a. 15 M b. .450 M c. 0.0930 M d. 0.555 M
1) A 110 mL solution of 0.340 M HCl(aq) is mixed with a solution of 330 mL of 0.150 M HNO3(aq). The solution is then diluted to a final volume of 1.00 L. How many moles of H+ are present in the final solution? 2) When 38.0 mL of 0.1250 M H2SO4 is added to 100 mL of a solution of Pblu, a precipitate of PbSO4 forms. The PbSO4 is then filtered from the solution, dried, and weighed. If the...
A volume of 69 mL of 0.080 M NaF is mixed with 23 mL of 0.20 M Sr(NO3)2. Calculate the concentrations of the following ions in the final solution.(Ksp for SrF2 2.0 × 10−10) [NO3−] M [Na+] M [Sr2+] M [F−] M