What is the ratio of the moles of sodium hydroxide to the moles of crystal violet (nNaOH/nCV+) at the start of the reaction? Make sure to account for the fact that different volumes of the stock solutions are mixed. 5.0 mL 2.0 × 10–5 M crystal violet solution 1.0 mL of 0.10 M NaOH solution

For the Equilibrium Reaction: Na++ Cl-= NaCl  When adding Saturated NaCl+ 12 M HCl  What stress is applied? What is the direction of the shift?   When adding Saturated NaCl+ 3M HCl What is the stress applied? What direction is the shift?

A student combines Fe(NO3)3 solution and KSCN solution to produce a solution in which the initial concentrations of Fe3+(aq) and SCN–(aq) are both 5.58 × 10–2 M. The chemical equilibrium forms FeSCN2+(aq):             Fe3+ + SCN- <=> FeSCN2+ The absorbance of this solution (from FeSCN2+) is measured as 0.161, and Beer's law equation (the trend line from best fitting) as Absorbance = 189 x Concentration of FeSCN2+ + 0.02 Determine the equilibrium concentration for SCN- in mol/L.

A solution contains 7.34x103 M sodium carbonate and 6.93x10-3 M ammonium iodide. Solid lead acetate is added slowly to this mixture. A. What is the formula of the substance that precipitates first? formula = B. What is the concentration of lead ion when this precipitation first begins? [Pb2*) =| M

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…

A solution was prepared in the lab when equal volumes of 3.00 × 10⁻⁴ M calcium chloride and 1.00 × 10⁻⁴ M lithium phosphate were combined.  A solution was prepared in the lab with equal volumes of 3.0 × 10⁻⁴ M calcium chloride and 1.00 × 10⁻⁴ M lithium phosphate. Evaluate the reaction quotient, Q, for calcium phosphate for these values.

Please don't provide handwritten solution

A solution contains 7.41×10-3 M lead nitrate and 6.81×10-3M silver acetate. Solid potassium sulfate is added slowly to this mixture.A. What is the formula of the substance that precipitates first? formula =   B. What is the concentration of sulfate ion when this precipitation first begins? [SO42-] = M

A student carries out the following titration by adding H2SO4.