A volume of 84 mL of 0.060 M NaF is mixed with 28 mL of .15...

A volume of 84 mL of 0.060 M NaF is mixed with 28 mL of .15 M Sr(NO3)2. Calculate the concentrations of the following ions in the final solution (Ksp for SrF2 is 2.0x10^-10)

Solutions

Expert Solution

queen_honey_blossom answered 2 days ago

Next > < Previous

Related Solutions

Assume that you mixed 20.00 mL of 0.040 M KI with 20.00 mL of 0.060 M...

Assume that you mixed 20.00 mL of 0.040 M KI with 20.00 mL of 0.060 M (NH4)2S2O8 , 10.00 mL of 0.00070 M Na2S2O3 , and a few drops of starch. The point of mixing sets time = 0. The Initial Concentrations are: [KI] = 0.016M [(NH4)2S2O8] = 0.024M [Na2S2O3] = 0.00014M Oxidation-Reduction Reaction between iodide and peroxydisulfate: 2I- + S2O8^2- -> 2SO4^2- + I2 Iodine Clock Method reaction: 2S2O3^2- +I2 -> 2I^- + S4O6^2- Question: The basis of the...

50 mL of 0.060 M K2CrO4 is mixed with 50 mL of 0.080 M AgNO3. Calculate...

50 mL of 0.060 M K2CrO4 is mixed with 50 mL of 0.080 M AgNO3. Calculate the following: a. The solubility of Ag2CrO4 (Ksp = 1.9 X 10-12) in the solution in moles per liter. b. The concentrations of the following ions Ag+, CrO4-2, K+, and NO3-.

a volume of 75mL of 0.040M NaF is mixed with 25mL of 0.10M Sr(NO3)2. Calculate the...

a volume of 75mL of 0.040M NaF is mixed with 25mL of 0.10M Sr(NO3)2. Calculate the concentration of the following ions in the final solution (Ksp for SrF2= 2.0x10^-10). [NO3-] [Na+] [Sr2+] [F-].

Denis titrates 25 mL of a 0.060 M solution of ammonia (NH3) with a 0.020 M...

Denis titrates 25 mL of a 0.060 M solution of ammonia (NH3) with a 0.020 M solution of hydrochloric acid. A) Write the chemical equation that occurs B) Do you expect the pH of the solution to be acidic, basic or neutral at the equivalence point? Explain. C) Calculate the pH after 20 mL of HCl solution have been added. Hint: Kb(NH3)=1.8*10-5

Calculate the pH of 100.0 mL of a buffer that is 0.060 M NH4Cl and 0.185...

Calculate the pH of 100.0 mL of a buffer that is 0.060 M NH4Cl and 0.185 M NH3 after the addition of 1.00 mL of 5.00 M HNO3.

A 360.0 −mL buffer solution is 0.170 M in HF and 0.170 M in NaF. A)...

A 360.0 −mL buffer solution is 0.170 M in HF and 0.170 M in NaF. A) What mass of NaOH could this buffer neutralize before the pH rises above 4.00? B) If the same volume of the buffer was 0.360 M in HF and 0.360 M in NaF, what mass of NaOH could be handled before the pH rises above 4.00? I keep getting 1.8 g and 3.5 g, which is wrong.

150.0 mL of 0.27 M HF with 230.0 mL of 0.32 M NaF Express your answer...

150.0 mL of 0.27 M HF with 230.0 mL of 0.32 M NaF Express your answer using two decimal places.

When 50.0 mL of 0.400 M Ca(NO3)2 is added to 50.0 mL of 0.800 M NaF,...

When 50.0 mL of 0.400 M Ca(NO3)2 is added to 50.0 mL of 0.800 M NaF, CaF2 precipitates, as shown in the net ionic equation below. The initial temperature of both solutions is 25.00°C. Assuming that the reaction goes to completion, and that the resulting solution has a mass of 100.00 g and a heat capacity the same as water, calculate the final temperature of the solution. Ca2+(aq) + 2 F-(aq) → CaF2(s) ΔH° = –11.5 kJ When trying to...

When 50.0 mL of 0.900 M Ca(NO3)2 is added to 50.0 mL of 1.80 M NaF,...

When 50.0 mL of 0.900 M Ca(NO3)2 is added to 50.0 mL of 1.80 M NaF, CaF2 precipitates, as shown in the net ionic equation below. The initial temperature of both solutions is 30.00°C. As the reaction proceeds, the temperature rises to 31.50 °C. Assuming that the reaction goes to completion, and that the resulting solution has a mass of 100.0 g and a specific heat of 4.18 J/(g ∙ °C), calculate the ΔH° for this reaction, expressed in kJ/mol...

When 50.0 mL of 0.400 M Ca(NO3)2 is added to 50.0 mL of 0.800 M NaF,...

When 50.0 mL of 0.400 M Ca(NO3)2 is added to 50.0 mL of 0.800 M NaF, CaF2 precipitates, as shown in the net ionic equation below. The initial temperature of both solutions is 30.00°C. Assuming that the reaction goes to completion, and that the resulting solution has a mass of 100.00 g and a specific heat of 4.18 J/(g ∙ °C), calculate the final temperature of the solution. Ca2+(aq) + 2 F-(aq) → CaF2(s) ΔH° = -11.5 kJ 30.55°C...

Subjects