Part 2 - Determining the Equilibrium [Fe(SCN)²+] 3690 :(2)9ms/ TABLE 3 Beaker A(1) A(2) Average A[Fe(SCN)2+]* AVS A/K 5 0.098 0.088 0.093 2.5x10-5 MS 6 0.154 0.142 0.148 4.01×10-s 7 0-174 8 9 0.178 0.176 4,8×105 0.230 0.232 0.231 6.3 × 10-5 0.291 0.294 0.2925 7.9×10-5 *This is calculated from average A and k from the previous part. Initial concentrations of iron (III) and thiocyanate ions *HINT: Use MIV1-M2V2 Total volume in each solution is 20.0 mL Mi 0.002 TABLE 4 Beaker [Fe3+]0 [SCN-] 0 5 0.001 2×104 6 0.001 4x164 7 0.001 6×104 8 0.001/8x104 9 0.001 10x104 12 VI 20 10mL 0.002 (2) = m (20) 0.002 (4) ~ SAT (svods 25 m2) క Fill out the following ICE tables to determine the equilibrium constant for each beaker. *HINTS: - For the "I" part of the table you will be using the initial concentrations calculated in TABLE 4 - For the "C" part of the table you will be using the Fe(SCN)2+ concentration in TABLE 3 [Fe(SCN)2+] - Ke [Fe3+][SCN] Part 2 - Determining the Equilibrium [Fe(SCN)²+] 3690 :(2)9ms/ TABLE 3 Beaker A(1) A(2) Average A[Fe(SCN)2+]* AVS A/K 5 0.098 0.088 0.093 2.5x10-5 MS 6 0.154 0.142 0.148 4.01×10-s 7 0-174 8 9 0.178 0.176 4,8×105 0.230 0.232 0.231 6.3 × 10-5 0.291 0.294 0.2925 7.9×10-5 *This is calculated from average A and k from the previous part. Initial concentrations of iron (III) and thiocyanate ions *HINT: Use MIV1-M2V2 Total volume in each solution is 20.0 mL Mi 0.002 TABLE 4 Beaker [Fe3+]0 [SCN-] 0 5 0.001 2×104 6 0.001 4x164 7 0.001 6×104 8 0.001/8x104 9 0.001 10x104 12 VI 20 10mL 0.002 (2) = m (20) 0.002 (4) ~ SAT (svods 25 m2) క Fill out the following ICE tables to determine the equilibrium constant for each beaker. *HINTS: - For the "I" part of the table you will be using the initial concentrations calculated in TABLE 4 - For the "C" part of the table you will be using the Fe(SCN)2+ concentration in TABLE 3 [Fe(SCN)2+] - Ke [Fe3+][SCN]

Balance each of the following neutralization reactions.   Part A HNO3(aq)+Zn(OH)2(s)→H2O(l)+Zn(NO3)2(aq)   Express your answer as a chemical equation. Identify all of the phases in your answer.

How many mL of liquid mercury with a density of 13.6g/mL must you dispense to have 1.56 x 10-3 mol

A chemist prepares a solution of vanadium(III) bromide (VBr) by measuring out 0.10 g of VBr3 into a 100. mL volumetric flask and filling to the mark with distilled water. Calculate the molarity of Br anions in the chemist's solution. Be sure your answer is rounded to 2 significant digits. mol L x10 X Ś

Explain your answer.

Can you please help me answer the homework

In the laboratory, a student adds 14.0 g of silver nitrate to a 375 mL volumetric flask and adds water to the mark on the neck of the flask. Calculate the concentration (in mol/L) of silver nitrate, the silver ion and the nitrate ion in the solution.

A student follows a lab protocol that asks them to make an ‘alcohol’ solution for an experiment. They make a 1.00 L solution by adding 575 g of an alcohol to water. Later they realize that there were three different alcohols sitting on the lab bench and they’re not sure which one they used. The alcohols are: methanol (CH3OH), ethanol (C2H5OH), and butanol (C4H9OH). They decide to boil the solution and they find that it boils at 106.40 °C. Using this information determine which alcohol the student used to make their solution. Density of water is 1.00 g/mL, Kb = 0.513 K/mc. Hint: you need to consider the molar masses of your alcohols.

Br (CH3)¿CuLi CuLi Br K H20 MgBr H20 M МоBr

A chemist prepares a solution of iron (III) chloride (FeC13) by measuring out 0.30 g of FeCl3 into a 300. mL volumetric flask and filling to the mark with distilled water. Calculate the molarity of Canions in the chemist's solution. Be sure your answer is rounded to 2 significant digits. mol L x10 X Ś