You are asked to double check the calculations for the % soda ash (Molar mass = 105.99 g/mol) in your sample. You have calculated the [NaOH] to be 0.10012 M anc the [HCI] to be 0.1007 M. Your lab partner prepared the soda ash sample by adding 2.352 g of unknown into 748.0 mL of distilled water. You prepared the sample by adding 28.0 mL of soda ash, 55.0 mL distilled water, 4 drops of phenolphthalein indicator and you filled the burette with HCI. The initial reading of the burette was 0.56 mL. The pink solution turned colourless at 21.92 mL and your lab partner note down the volume of 43.81 mL for the second inflection point. Looking at the following set up below, how many errors are present from the information present above? [(0.1012 M) x (0.4325 L) x (1/2) (105.99 g/mol)]| 07 a 4 -T 100%

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You perform a titration on 11.35 mL of an HCl solution of unknown concentration. It requires 75.25 mL of 0.285 M NaOH to turn slightly pink. What is the concentration of the HCl (in M)?

Calculate the molarity of a NaOH solution if 25.85 mL of NaOH is titrated with 0.425 grams of KHP and 2.15 mL of 0.140M HCI is required.

An unknown acid salt was dissolved in water and titrated with 0.105 M NaOH. If 1.20 grams of the salt were dissolved and it took 120 mL to reach the equivalence point, what is the unknown?

A 15.00mL sample of ammonium hydroxide (0.980g/mL) is titrated with 31.25mL of0.500M HCl. Find the molarity and mass percent of the ammonium hydroxidesolution. Be sure to start with a balanced equation.

Some soluble compounds are listed in the table below. Complete the table by filling in the name or chemical formula of each compound, whichever is missing. (If there is more than one way to name the compound, choose the name used when the compound is dissolved in water.) Also classify the compound using the checkboxes. compound 0 HCH₂ CO₂ NH3 HCIO4 name barium hydroxide 0 0 type of compound (check all that apply) strong weak strong weak acid base base acid ionic molecular 0 0 0 0 X S

By titration, it is found that 36.7 mL of 0.117 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the concentration of the HCl solution.  I got 0.14862 - but is wrong.

be = MULTIPLE CHOICE QUESTION You perform a titration using a 0.198 M concentration of Ba(OH)2 as the base against 25.00 mL of nitrous acid (HNO₂). You found that you needed 18.85 mL of Ba(OH)2 to reach the end point of the reaction. How many moles of nitrous acid do you have? HINT: You need to write the balanced chemical equation for the reaction between Ba(OH)2 and HNO2. 0.00736 mol of HNO₂ 0.00373 mol of HNO2 (Mole (unit) - Wikipedia 0.00187 mol of HNO2 Rewatch Submit

Consider the reaction between 50.0 mL of 0.10 M NaOH and 75.0 mL of 0.20 M HCI at 25°. Which of the following statements is TRUE? HCl is the limiting reactant. After the reaction, the concentration of Na* is equal to the concentration of Cl'. After the reaction, the concentration of Cl' is still 0.200 M because Cl' is a spectator ion. After the reaction, the concentration of Na* is greater than the concentration of H30*. The final solution has a pH 1.10.