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What is the pH of 0.5M FeCl3?
I am assuming that this FeCl3 is going to be aqueous, as it usually is. Therefore, Fe+3 forms complexes in water in the following manner: B FeCl3(aq) +6H2O → [Fe(H2O)6]3+ Now, because the Fe has a positive charge, it will pull the negative electron cloud towards itself, making the bond holding the H on the OH weaker, which leads to an easier release of protons (H+). Therefore, [Fe(H2O)6]3+ → [Fe(H2O)5]+2 + H+ As you can see, Fe is in the "net reaction" acting as an acid, as it makes the H2O's bound to it release H+ ions into the water. Therefore, FeCl3 is assigned a Ka value, which = 2.0 x 10-3. Now, we need to set up our table: FeCl3 → Fe(H2O)5]+2 + H+ Initial concentration 0.5 M 0.0 M 0.0 M Change (-) x x x Final Concentration 0.5-x x x So, we can set up our equilibrium constant expression: Ka= [H+][ [Fe(H2O)5]+2]/[[Fe(H2O)6]3+] we know Ka therefore: 2.0 x 10-3= x2/0.5-x Solve for x, must use quadratic: 0.001-2.0 x 10-3x-x2=0 Solving the quadratic gives us: x= -0.032639, 0.030639 The negative result is unphysical, because we cannot have a negative concentration, therefore, x= 0.030639, which from our graph tells us that the concentration of H+ = 0.030639M, so to find the pH: -log( 0.030639)= pH = 1.51, so therefore, the pH of 0.5 M FeCl3 is 1.51. Hope that helps, don't know if you needed to know all the details. Praise God! Eugene.
How many moles of HCL in 50ml of 1.0 M HCL?
50ml = .05L of HCL 1.0 M = 1mol / 1L of HCL simply multiply - .05 by 1.0, and get your answer!
How much gram of fecl3 to be used in preparing fecl3 solution for testing citric acid in semen?
The amount of FeCl3 needed depends on the concentration of the FeCl3 solution required for the test. Typically, a 2-5% solution of FeCl3 is used. To make a 100mL of 2-5% FeCl3 solution, you would need to dissolve 2-5 grams of FeCl3 in distilled water. The exact amount can be calculated using the formula: (desired % concentration/100) x volume of solution needed x molar mass of FeCl3.
How many moles of zn are consumed when 1.60 x 1024 molecules of hcl react completely in the following equation zn plus 2hcl equals zncl2 plus h2?
1 mole of Zn reacts with 2 moles of HCl. Thus, 1.60 x 10^24 molecules of HCl is equivalent to 0.8 x 10^24 moles of HCl. Since the mole ratio is 1:1 between Zn and HCl, 0.8 x 10^24 moles of Zn are consumed in the reaction.
What is the pH of CH3NH3Cl?
CH3NH3Cl->CH3NH3+ + Cl¯ Cl¯+H2O-> Doesn't reactor! CH3NH3+ +H2O <-> CH3NH2 + H3O+ (c-x) M x M x M H2O + H2O <-> H3O+ + OH¯ y M y M [H3O+]w= (x+y) M [OH¯]= y M Like this: [H3O+]>[OH¯] => Acid
How many milliliters of 0.200 M FeCl3 are needed to react with an excess of Na2S to produce 2.75 g of Fe2S3 if the percent yield for the reaction is 65.0 percent?
.2M x V FeCl3=moles FeCl3 x 1mole Fe2S3/2mole FeCl3=moles of Fe2S3 x mm of Fe2S3/1 mole Fe2S3= g Fe2S3 x .65% yield. 2.75g Fe2S3/ .65= 4.23g Fe2S3/ 207.91= .02035 x 2mole FeCl3=.0407 moles FeCl3/ .2M FeCl3= .2035 L x 1000= 203.5 ml
What is the pH of 0.5M FeCl3?
I am assuming that this FeCl3 is going to be aqueous, as it usually is. Therefore, Fe+3 forms complexes in water in the following manner: B FeCl3(aq) +6H2O → [Fe(H2O)6]3+ Now, because the Fe has a positive charge, it will pull the negative electron cloud towards itself, making the bond holding the H on the OH weaker, which leads to an easier release of protons (H+). Therefore, [Fe(H2O)6]3+ → [Fe(H2O)5]+2 + H+ As you can see, Fe is in the "net reaction" acting as an acid, as it makes the H2O's bound to it release H+ ions into the water. Therefore, FeCl3 is assigned a Ka value, which = 2.0 x 10-3. Now, we need to set up our table: FeCl3 → Fe(H2O)5]+2 + H+ Initial concentration 0.5 M 0.0 M 0.0 M Change (-) x x x Final Concentration 0.5-x x x So, we can set up our equilibrium constant expression: Ka= [H+][ [Fe(H2O)5]+2]/[[Fe(H2O)6]3+] we know Ka therefore: 2.0 x 10-3= x2/0.5-x Solve for x, must use quadratic: 0.001-2.0 x 10-3x-x2=0 Solving the quadratic gives us: x= -0.032639, 0.030639 The negative result is unphysical, because we cannot have a negative concentration, therefore, x= 0.030639, which from our graph tells us that the concentration of H+ = 0.030639M, so to find the pH: -log( 0.030639)= pH = 1.51, so therefore, the pH of 0.5 M FeCl3 is 1.51. Hope that helps, don't know if you needed to know all the details. Praise God! Eugene.
How many moles of HCL in 50ml of 1.0 M HCL?
50ml = .05L of HCL 1.0 M = 1mol / 1L of HCL simply multiply - .05 by 1.0, and get your answer!
How much gram of fecl3 to be used in preparing fecl3 solution for testing citric acid in semen?
The amount of FeCl3 needed depends on the concentration of the FeCl3 solution required for the test. Typically, a 2-5% solution of FeCl3 is used. To make a 100mL of 2-5% FeCl3 solution, you would need to dissolve 2-5 grams of FeCl3 in distilled water. The exact amount can be calculated using the formula: (desired % concentration/100) x volume of solution needed x molar mass of FeCl3.
What is the HCl concentration if 53.1 mL of 0.300 M NaOH is required to titrate a 15.0 mL sample of the acid?
HCl + NaOH ---> NaCl + H2O(53.1 ml)(0.300 M) = (15.0 ml)(x M)x = 1.06 M
How many moles of zn are consumed when 1.60 x 1024 molecules of hcl react completely in the following equation zn plus 2hcl equals zncl2 plus h2?
1 mole of Zn reacts with 2 moles of HCl. Thus, 1.60 x 10^24 molecules of HCl is equivalent to 0.8 x 10^24 moles of HCl. Since the mole ratio is 1:1 between Zn and HCl, 0.8 x 10^24 moles of Zn are consumed in the reaction.
What is the pH of CH3NH3Cl?
CH3NH3Cl->CH3NH3+ + Cl¯ Cl¯+H2O-> Doesn't reactor! CH3NH3+ +H2O <-> CH3NH2 + H3O+ (c-x) M x M x M H2O + H2O <-> H3O+ + OH¯ y M y M [H3O+]w= (x+y) M [OH¯]= y M Like this: [H3O+]>[OH¯] => Acid
If 25.00ml of 50m naoh is used to titrate 26.25ml of hcl to the equivalence point what is the concentration of the hcl?
First balance the equation of the reaction: NaOH + HCl ---> NaOH + H2O The ratio of moles is 1:1 M1V1 = M2V2 (molarity1 x volume1) = (molarity2 x volume2) M2 = M1V1 / V2 molarity2 = (molarity1 x volume1) / (volume2) M of HCl = 50M x 0.025 litres / 0.02625 litres = 47.6 M
A solution of HCl has H plus equals 5.5 x 10-4 What is the pH of this solution?
apexvs answer 3.3
What is the product of Fe plus O2 plus H2O?
Hydrated Iron (III) oxide: 2Fe + 1.5O2 + xH2O -> Fe2O3·xH2O where x is the number of H2O molecules present.
How many grams of HCL needed to react with 4000 g of Na2co3?
The balanced chemical equation for this reaction is 2 HCl + Na2CO3 -> 2 NaCl + H2O + CO2. From the equation, 1 mole of Na2CO3 reacts with 2 moles of HCl. Calculate the number of moles of Na2CO3 in 4000g, then use the mole ratio to find the moles of HCl needed. Finally, convert moles of HCl to grams.
What is the molarity of an hcl solution if 7ml hcl solution is titrated with 27.6ml of 0.170m of naoh solution?
The balanced chemical equation for the reaction is: HCl + NaOH -> NaCl + H2O. From the equation, it is a 1:1 mole ratio reaction. Therefore, the moles of HCl can be calculated from the volume and concentration of NaOH used in the titration. Then, use the moles of HCl and the volume of HCl solution used to calculate the molarity of the HCl solution.
