Question

In: Chemistry

A chemist prepares a solution of mercury(I) chloride Hg2Cl2 by measuring out 0.0000059μmol of mercury(I) chloride...

A chemist prepares a solution of mercury(I) chloride Hg2Cl2 by measuring out 0.0000059μmol of mercury(I) chloride into a 50.mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in mol/L of the chemist's mercury(I) chloride solution. Round your answer to 2 significant digits.

Solutions

Expert Solution

volume of solution = 50ml   = 0.05L

no of moles of mercury(I) chloride Hg2Cl2    = 0.0000059μmol    

                                                               = 0.0000059*10^-6mol                   [ μmol    = 10^-6 mol]

molarity   = no of moles/volume of solution in L

              = 0.0000059*10^-6mol/0.05L

               = 1.2*10^-10mol/L >>>>answer

the concentration in mol/L of the chemist's mercury(I) chloride solution= 1.2*10^-10 mol/L

queen_honey_blossom answered 2 years ago
Next > < Previous

Related Solutions

Because of the toxicity of mercury compounds, mercury(I) chloride is used in antibacterial salves. The mercury(I)...
Because of the toxicity of mercury compounds, mercury(I) chloride is used in antibacterial salves. The mercury(I) ion (Hg2 2+ ) consists of two bound Hg+ ions. a. What is the chemical formula of mercury(I) chloride? (1 mark) b. Calculate [Hg2 2+ ] in a saturated solution of mercury(I) chloride (Ksp = 1.5 x 10-18 ). c. Seawater contains 0.03 kg of NaCl per litre. Using a suitable approximation, find [Hg2 2+ ] if the seawater is saturated with mercury(I) chloride....
If a compound pharmacist prepares 3.0L of a solution containing 0.8325g of calcium chloride, what is...
If a compound pharmacist prepares 3.0L of a solution containing 0.8325g of calcium chloride, what is the concentration of calcium ions in solution in mEq/L? (note: 1Eq = 1000 mEq).
Suppose the Chemist weighs out a 5.931g sample of the standard sodium chloride (formula Weight 58.44)...
Suppose the Chemist weighs out a 5.931g sample of the standard sodium chloride (formula Weight 58.44) and dissolves it in water to make exactly one litre of solution. what is the actual mass of the sodium chloride in the sample. please help its due in 2 hrs
When solutions of silver nitrate and magnesium chloride are mixed, silver chloride precipitates out of solution...
When solutions of silver nitrate and magnesium chloride are mixed, silver chloride precipitates out of solution according to the equation 2AgNO3(aq)+MgCl2(aq)→2AgCl(s)+Mg(NO3)2(aq) Part A What mass of silver chloride can be produced from 2.00 L of a 0.163 M solution of silver nitrate? Express your answer with the appropriate units. Part B The reaction described in Part A required 3.39 L of magnesium chloride. What is the concentration of this magnesium chloride solution?
When solutions of silver nitrate and calcium chloride are mixed, silver chloride precipitates out of solution...
When solutions of silver nitrate and calcium chloride are mixed, silver chloride precipitates out of solution according to the equation 2AgNO3(aq)+CaCl2(aq)→2AgCl(s)+Ca(NO3)2(aq) What mass of silver chloride can be produced from 1.51 L of a 0.201 M solution of silver nitrate? Express your answer with the appropriate units. The reaction described in Part A required 3.51 L of calcium chloride. What is the concentration of this calcium chloride solution? Express your answer with the appropriate units.
When solutions of silver nitrate and calcium chloride are mixed, silver chloride precipitates out of solution...
When solutions of silver nitrate and calcium chloride are mixed, silver chloride precipitates out of solution according to the equation 2AgNO3(aq)+CaCl2(aq)?2AgCl(s)+Ca(NO3)2(aq) Part A What mass of silver chloride can be produced from 1.35L of a 0.166M solution of silver nitrate? Express your answer with the appropriate units. mass of AgCl = SubmitHintsMy AnswersGive UpReview Part Incorrect; Try Again; 5 attempts remaining Part B The reaction described in Part A required 3.38L of calcium chloride. What is the concentration of this...
Consider the electrochemical reactions shown below. Mercury(I) chloride, also known as calomel, is a solid used...
Consider the electrochemical reactions shown below. Mercury(I) chloride, also known as calomel, is a solid used in reference electrodes. The two reactions are Zn = Zn2+ + 2e- Hg2Cl2 + 2e- = 2Cl- + 2Hg What is the overall chemical reaction? Develop an expression for U, the equilibrium potential of the cell. Write down an expression for the standard potential of the cell in terms of the standard Gibbs energies of formation. Use standard half-cell potentials from the table to...
reaction: potassium chloride with mercury nitrate KCl + Hg2(NO3)2
reaction: potassium chloride with mercury nitrate KCl + Hg2(NO3)2
Mercury(I) oxide decomposes into elemental mercury and elemental oxygen:
Mercury(I) oxide decomposes into elemental mercury and elemental oxygen:.(a)Write the equilibrium-constant expression for this reaction in terms of partial pressures.(b) Suppose you run this reaction in a solvent that dissolves elemental mercury and elemental oxygen. Rewrite the equilibrium-constant expression in terms of molarities for the reaction, using (solv) to indicate solvation.
A chemist at a pharmaceutical company is measuring equilibrium constants for reactions in which drug candidate...
A chemist at a pharmaceutical company is measuring equilibrium constants for reactions in which drug candidate molecules bind to a protein involved in cancer. The drug molecules bind the protein in a 1:1 ratio to form a drug-protein complex. The protein concentration in aqueous solution at 25 ∘C is 1.78×10−6 M . Drug A is introduced into the protein solution at an initial concentration of 2.00×10−6M. Drug B is introduced into a separate, identical protein solution at an initial concentration...
ADVERTISEMENT
Subjects
ADVERTISEMENT
Latest Questions
ADVERTISEMENT