A saline solution contains 1.00 g of NaCl (molar mass = 58.55 g/mol) in 75.8 mL of solution. Calculate the concentration of NaCl in this solution, in units of molarity. Express the concentration in molarity to three significant figures.
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- original molarity= .548 A 5.00 mL sample of this KOH solution is added to a 100 mL volumetric flask, and water is added to the mark. What is the new molarity of K+ ions in this solution?The molarity of naoh is 0.1715Determine the molarity of 3.72 moles of NaBr in 575mL of solution. (MM NaBr= 102.89 g/mol) Report your answer to 3 significant figures. Do not include the unit when writing your answer.
- What mass of sodium glycolate (NaC2H3O3) should be added to 400.0 mL of 1.00 M glycolic acid to produce a buffer solution with a pH of 4.00? Ka = 1.47 x 10-4. Please indicate the full solutions.A buffer contains 0.015 mol of lactic acid (pK₁ = 3.86) and 0.080 mol of sodium lactate per liter. H₂C OH Lactic acid OH Calculate the pH of the buffer. H₂C. Calculate the change in pH after adding 9.0 mL of 0.10 M HCl to 1.0 L of the buffer. O OH Sodium lactate Calculate the change in pH after adding 9.0 mL of 0.10 M HCl to 1.0 L of pure water. O Na+ buffer pH: buffer pH change: water pH change: units unitsIf your 16x concentrated stock solution contains 20g of NaCl per liter, how much Nacl would one liter of your working solution contain? Round your result to 2 decimal points. g of Nacl
- What mass of sodium glycolate (NaC2H3O3) should be added to 400.0 mL of 1.00 M glycolic acid to produce a buffer solution with a pH of 4.00? Ka = 1.47 x 10-4What would you expect to see if you were to create a solution that has 20.0 grams of the NaCl and the solubility is 35.0 g in 100 mL? What type of solution is this? Format B I U ... >Calculate the following concentration given this