How to prepare these solutions?   250.0 mL 0.125 M stock Na2S2O3 solution from Na2S2O3·5H2O crystals  250 mL 0.10 M NaOH NOTE: Use the 1.0 M NaOH prepared 250.0 mL standard 2500 ppm Cu(II) stock solution

When aqueous solutions of AgNO3 and NaCl are mixed together, the precipitate that will form is Solubility of KCl at 20 oC is 34 g/100 g H₂O. A solution containing 20 g of KCI in 50 g of water at 20 oC is classified as solution. NH3 will dissolve in water because NH3 is a solvent. solute. CCl4 is insoluble in water because water is a

A 2.45 g mixture of BaCl2 and Ba(NO3)2 is dissolved in water.  Excess AgNO3 is added and all of the dissolved chloride ion is precipitated. The resulting precipitate weighs 0.845 g.  Use the following Molar Masses (in g mol−−1) as required: Ba: 137.3 Cl:  35.45 Ag: 107.9 N: 14.01 O: 16.00   What is the mass of Ba(NO3)2 in the original mixture?  Enter a mass accurate to three significant figures.  g

A solution contains 1.43x10 M lead nitrate and 5.74x10 M silver acetate. Solid potassium sulfate is added slowly to this mixture. A. What is the formula of the substance that precipitates first? 18 formula = B. What is the concentration of sulfate ion when this precipitation first begins? [so,)=| M

Consider the following equilibrium: Cu²+ (aq) + 4NH3(aq) Cu(NH3)4²+₁ (aq) (Kf = 4.8e+12) A solution is made by mixing 15.0 mL of 0.90 M CuSO4 and 1.00 L of 0.530 M NH3. Assume additive volumes to answer the following questions. Give all answers to three sig figs. a) What is the concentration of NH3 in the resulting solution? [NH3] = .47 M b) What is the concentration of Cu(NH3)42+ in the resulting solution? [Cu(NH3)4²+] = 5.3e-2 X M c) What is the concentration of Cu²+ in the resulting solution? [Cu²+] = 5.3e-2 X M

The solubility of magnesium fluoride,MgF2​, in water is1.5×10−2 g/L. What is the solubility (in grams per liter) of magnesium fluoride in0.31Mof sodium fluoride,NaF?Solubility = \[ g / L \] 10 item attempts remaining

Determine the mass of potassium bromide necessary to precipitate all of the Cu^+ in 305 mL solution that is 1.6 M Cu ^+. The ksp of CuBr is 5.3*10^-9

9

The flask contains 10.0 mL10.0 mL of HClHCl and a few drops of phenolphthalein indicator. The buret contains 0.110 M NaOH.0.110 M NaOH. It requires 31.4 mL31.4 mL of the NaOHNaOH solution to reach the end point of the titration. What is the initial concentration of HClHCl?

Suggest a reason why it is desirable to use an excess of barium ion in the precipitation.