Q: The mass of calcium sulfate that is dissolved in 175 mL of a saturated solution is
A: Consider the given information is as follows; Volume of solution = 175 mL = 0.175 L Mass of calcium…
Q: What volume of a 0.167 M KBr solution is needed to provide 18.5 g of KBr?
A: The number of moles (n) in 18.5 g of KBr is calculated using equation (1) in which m and M…
Q: How many milliliters of 10.0M HCI(aq) are needed to prepare 300.0 mL of 1.00 M HCI(aq)? mL V =
A: Dilution of the solution: When we dilute a concentrated solution with pure water, the mole of solute…
Q: How many grams of HCl are there in 350.0 mL of 0.112 M solution?
A: Given: Volume of HCl = 350.0 mL = 0.350 L Concentration of HCl = 0.112 M Molar mass of HCl = 36.46…
Q: solution of Kl?
A: The reactants given are Pb(NO3)2 and KI.
Q: what is the mass of KHP in unknown and what is thr percent KHP in unknown?
A: mL of NaOH used = 14.4 mL = 0.0144 Lconcentration of NaOH = 0.1152 M = 0.1152 mol/Lmoles of NaOH…
Q: Which combinations of solutions will lead to the formation of a precipitate?
A:
Q: to prepare 0.1 L of 0.1 N from 0.2N HCI we need to
A:
Q: A solution is prepared by dissolving 20 mL of pure hydrogen peroxide in enough water to make 200 mL…
A:
Q: g solution
A: When strong acid mixed with strong base then completely neutralization occur because both are strong…
Q: Which produces the greatest number of ions when one mole dissolves in water?
A:
Q: How is a titration used to determine the concentration of an acid or base?
A: Acid base titration is used for quantitative analysis in determining the concentration of unknown…
Q: Calcium bydroxide may be used to neutralize (completely react with) aqueous hydrochlcric acid.…
A: The balanced reaction will look like, 2HCl + Ca(OH)2 → CaCl2 + 2H2O It is given that,amount of solid…
Q: ___ Na + ___ F2 → ___ NaF balance the equation
A: In a balanced equation no.of atoms in both side (reactants and products) should be equal. In a…
Q: If 25.0 mL of a 1.00 M HCI solution is diluted to 2.00 L, what is the molarity of the new solution?
A: Given :- initial molarity of solution = 1.00 M initial volume of solution = 25.0 mL…
Q: K of an Indicator ReporT sheet Name
A: To determine the Corresponding value of KHAc & kHIN
Q: Convert the concentration of 0.700 M Na,SO, to g/mL
A: We use molar mass, which is a gram per mole. Molarity x molar mass = moles/litre x grams /mole the…
Q: If equal volumes of 6 M sulfuric acid and distilled water are added together, what is the…
A: given concentration of sulfuric acid = 6.0 M And we mixed the equal volume of distilled water and…
Q: moles of HCI were consumed by the tablet and 0.0120 moles of HCI were initial les of NaOH were…
A: Excess Moles of HCl = = 0.0120 - 0.01031 = 0.00169 mol
Q: What is the concentration of cobalt in mM?
A: The data given is,
Q: Can the concentration of ions in solution ever be greater than the concentration of solute? Why or…
A: The concentration of a solution is the ratio between the amount of solute and the amount of…
Q: the final volume equals the initial volume of the solution plus the volume of NaOH solution added. ?
A: Given, Molarity of Acid(M) = 0.4500 M Volume of Acid(V) = 78.9 mL mmol of Acid = M × V = 0.4500 ×…
Q: 0.946 L). (b) How many milliliters of the muriatic acid solution contain 9.66 g of HC1?
A:
Q: A 13.0 mL sample of an unknown H3PO4 solution requires 122 mL of 0.140 M KOH to completely react…
A: Given information: Volume of unknown H3PO4 solution = 13.0 mL Volume of KOH = 122 mL Concentration…
Q: what happens at the molecular level when one substance dissolves into another?
A: When one substance gets dissolved in another, the substance which gets dissolved is called as…
Q: How many grams of pure sodium carbonate are needed to standardize a 0.20 N HCl when you expect the…
A: Given that - Normality of HCl = 0.20 N Volume of HCl used = 25.0 mL Then mass of HCl can be…
Q: 0.13865N HCl (500 mL) will be prepared from 12N HCl solution.
A: Given- N1=0.13865 V1=500mL N2=12N V2=?
Q: What is the final concentration of a solution prepared by diluting 35.0 mL of 12.0 M HCl to a final…
A:
Q: What is the concentration of HNO3 if 9.80×10-2 mol are present in 775 mL of the solution?
A: Molarity is one of the ways to express the concentration of solution We are required to find the…
Q: concentration of Nal in the resulting solution?
A: The ratio of moles of solute to the volume of solution in liters is known as molarity. Given…
Q: 2NaCl + Pb(NO3)2 → 2NANO3 + PbCl2 How many mL of 0.237 M NaCl react with 39.1 mL of 0.126 M…
A:
Q: molar concentration of
A:
Q: The concentration of th.
A:
Q: How many moles of precipitate will be formed when 70.0 mL of .150 M AgNO3
A: You have molarity of AgNO3 = 0.15 M Volume of AgNO3 = 70.0 mL = 0.07 L You know that Precipitation…
Q: Q: How many grams of precipitate are formed when 35 mL of 0.25 M zinc chloride solution is mixed…
A: Given : Concentration of sodium phosphate i.e Na3PO4 = 0.20 M Volume of Na3PO4 solution = 25 mL =…
Q: How many moles of potassium chloride are needed to precipitate all the lead(II) ion from 19.0 mL of…
A: Given: Volume of lead(II) nitrate is 19.0 mL Molarity of Lead (II) nitrate is 0.450 M The reaction…
Q: How many grams of pure sodium carbonate are needed to standardize a 0.1045N HCl when you expect the…
A: Given-> Normality of HCl = 0.1045 N = 0.1045 M (For HCl , molarity = normality) Volume of HCl =…
Q: What is the solution of 113g to ug?
A: Here given, 113 g We know the formula for converting gram to microgram is--- 1 gram = 1000000…
Q: What mass of sodium carbonate is required to precipitate all of the lead ions from 80.0 mL of 0.100…
A: Lead nitrate reacts with sodium carbonate to form lead carbonate as precipitate. Net Ionic Equation…
Q: True or false: the determination of a molar mass of a compound by the titration method used today…
A: True. The determination of a molar mass of a compound by the titration method used today depends on…
Q: A saturated solution ________.
A: Solution is the mixture of solvent and solute particles. In solution, solvent is present at greater…
Q: what is a soluble reactivity shim?
A: Soluble poisons are called chemical shim, produce a spatially uniform neutron absorption when…
Q: Given the following concentration in molar units calculate the concentration in mg/L. 0.066 M H2SO4
A:
Q: A 100 mL sample contains 88.9 ng As. What is the concentration of As (ppb) if its density is 1.20…
A:
Q: How many moles of Agl will be formed when 75.0ml of 0.300 M AgNo3 is completely reacted according to…
A:
Q: What volume of 0.200 M ethanol solution contain of thefollowing amounts? 1.22 mol ethanol
A: Given: The moles of ethanol are 1.22 mol. The volume of the ethanol solution is 0.200 M .
Q: What is the mass of the of the Ba(NO3)2 needed to make the 200 mL of the 0.01 M solution?
A:
Q: Express this concentration in ppb.
A:
Q: A 2400. gram sample of an aqueous solution contains 0.012 grams of NH3. What is the concentration of…
A: Given solution has mass 2400 g and it contains 0.012 g of NH3 (which is solute).
Trending now
This is a popular solution!
Step by step
Solved in 2 steps with 1 images
- In the reaction in Exercise 12.33, another trial was carried out. The reaction began with an initial concentration of N2 equal to the initial concentration of NO. Each had a concentration of 0.100 mol L-1. WTat were the equilibrium concentrations of all species? The following reaction establishes equilibrium at 2000 K: N2(g) + O2(g) ^2 NO K = 4.1 X 10~4 If the reaction began with 0.100 mol L-1 of N2 and 0.100 mol L'1 ofO2, what were the equilibrium concentrations of all species?The following question is taken from a Chemistry Advanced Placement Examination and is used with the permission of the Educational Testing Service. Solve the following problem: MgF2(s)Mg2+(aq)+2F(aq) In a saturated solution of MgF2 at 18 C, the concentration of Mg2+ is 1.21103M . The equilibrium is represented by the preceding equation. (a) Write the expression for the solubility-product constant, Ksp, and calculate its value at 18 C. (b) Calculate the equilibrium concentration of Mg2+ in 1.000 L of saturated MgF2 solution at 18 C to which 0.100 mol of solid KF has been added. The KF dissolves completely. Assume the volume change is negligible. (c) Predict whether a precipitate of MgF2 will form when 100.0 mL of a 3.00103 -M solution of Mg(NO3)2 is mixed with 200.0 mL of a .2.00103 -M solution of NaF at 18 C. Show the calculations to support your prediction.. (d) At 27 C the concentration of Mg2+ in a saturated solution of MgF2 is 1.17103M . Is the dissolving of MgF2 in water all endothermic or an exothermic process? Give an explanation to support your conclusion.Again the experiment in Exercise 12.33 was redesigned. This time, 0.15 mol each of N, and O2 was injected into a 5.0-L container at 2500 K, at which the equilibrium constant is 3.6 X 10-?. What was the composition of the reaction mixture at equilibrium? l'he following reaction establishes equilibrium at 2000 K: N2(g) + O2(g) *2 2 NO K = 4.1 X IO-4 If the reaction began with 0.100 mol L-1 of N2 and 0.100 mol L-’ ofO2, what were the equilibrium concentrations of all species?
- The experiment in Exercise 12.33 was redesigned so that the reaction started with 0.15 mol each of N2 and O2 being injected into a 1.0-L container at 2500 K. The equilibrium constant at 2500 K is 3.6 X 10“’. What was the composition of the reaction mixture after equilibrium was attained? The following reaction establishes equilibrium at 2000 K: N2(g) + O2(g) *2 2 NO K = 4.1 X IO-4 If the reaction began with 0.100 mol L-1 of N2 and 0.100 mol L-’ ofO2, what were the equilibrium concentrations of all species?Nitrogen, hydrogen, and ammonia are in equilibrium in a 1000-L reactor at 550 K. The concentration of N2 is 0.00485 M, H2 is 0.022 M, and NH3 is 0.0016 M. The volume of the container is halved, to 500 L. (a) Calculate the equilibrium constant. (b) Define y as the change in the concentration of nitrogen in the 500-L container. Is y positive or negative? (c) Write the iCe table and express the equilibrium constant in a polynomial in terms of y.How is the strength of an acid related to the position of its ionization equilibrium? Write the equations for the dissociation (ionization) of HCI, HNO3, and HClO4in water. Since all these acids are strong acids, what does this indicate about the basicity of the Cl-, NO3, and ClO4ions? Are aqueous solutions of NaCl, NaNO3, or NaClO4basic?
- Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go a step further and examine the equilibrium between carbonate ion and CaCOj. The reaction is Ca2+(aq) + COj2_(aq) ** CaCO,(s) The equilibrium constant for this reaction is 2.1 X 10*. If the initial calcium ion concentration is 0.02 AI and the carbonate concentration is 0.03 AI, what are the equilibrium concentrations of the ions? A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H2COj(aq) H+(aq) + HCO}‘(aq) K = 4.4 X 10"7 She starts with 0.1000 AI carbonic acid. What are the concentrations of all species at equilibrium?What is Le Chteliers principle? Consider the reaction 2NOCI(g)2NO(g)+Cl2(g) If this reaction is at equilibrium. what happens when the following changes occur? a. NOCI(g) is added. b. NO(g) is added. c. NOCI(g) is removed. d. Cl2(g) is removed. e. The container volume is decreased. For each of these changes, what happens to the value of K for the reaction as equilibrium is reached again? Give an example of a reaction for which the addition or removal of one of the reactants or products has no effect on the equilibrium position. In general, how will the equilibrium position of a gas-phase reaction be affected if the volume of the reaction vessel changes? Are there reactions that will not have their equilibria shifted by a change in volume? Explain. Why does changing the pressure in a rigid container by adding an inert gas not shift the equilibrium position for a gas-phase reaction?For the reactionH2(g)+I2(g)2HI(g), consider two possibilities: (a) you mix 0.5 mole of each reactant. allow the system to come to equilibrium, and then add another mole of H2 and allow the system to reach equilibrium again. or (b) you mix 1.5 moles of H2 and 0.5 mole of I2 and allow the system to reach equilibrium. Will the final equilibrium mixture be different for the two procedures? Explain.
- Suppose a reaction has the equilibrium constant K = 1.7 108 at a particular temperature. Will there be a large or small amount of unreacted starting material present when this reaction reaches equilibrium? Is this reaction likely to be a good source of products at this temperature?Because carbonic acid undergoes a second ionization, the student in Exercise 12.39 is concerned that the hydrogen ion concentration she calculated is not correct. She looks up the equilibrium constant for the reaction HCO,-(aq) «=* H+(aq) + COf'(aq) Upon finding that the equilibrium constant for this reaction is 4.8 X 10“H, she decides that her answer in Exercise 12.39 is correct. Explain her reasoning. A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H,CO,(aq) 5=6 H+(aq) + HCO,'(aq) K = 4.4 X 10'7She starts with 0.1000 A1 carbonic acid. W hat are the concentrations of all species at equilibrium?. Lead(II) chloride, PbCl2(s), dissolves in water to the extent of approximately 3.6102Mat 20 °C. Calculate Kspfor PbCl2(s), and calculate its solubility in grams per liter.