Given the following information: formic acid Ka = 1.8E-4 HCOOH HCIO hypochlorous acid Ka = 3.5E-8 (1) Write the net ionic equation for the reaction that occurs when equal volumes of 0.372 M aqueous formic acid and sodium hypochlorite are mixed. It is not necessary to include states such as (aq) or (s). Use HCOO as the formula for the formate ion. A₂ A² A₂ A² A₂ A² A₂ A² (2) At equilibrium the ✓ will be favored. (3) The pH of the resulting solution will be V seven.

Sodium hydrogen carbonate (NaHCO,), also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid (HCl) , which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO, neutralizes excess HCl through this reaction: HCl(aq) + NaHCO3(aq) → NaCl(aq) + H2O(1) + Co,(g) The CO, gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a man suffering from indigestion can be considered to be 250. mL of a 0.088 M HCl solution. What mass of NaHCO, would he need to ingest to neutralize this much HCl ? Be sure your answer has the correct number of significant digits.

Sodium hydrogen carbonate NaHCO3, also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid HCl, which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO3 neutralizes excess HCl through this reaction: HCl(aq)+NaHCO3(aq)→NaCl(aq)+H2O(l)+CO2(g)  The CO2 gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a woman suffering from indigestion can be considered to be 200.mL of a 0.089M HCl solution. What mass of NaHCO3 would she need to ingest to neutralize this much HCl? Be sure your answer has the correct number of significant digits.

A solution of sodium hydroxide is standardized against potassium hydrogen phthalate (molecular mass = 204.224 g mol-1). From the following data, calculate the molarity of the NaOH solution. The mass of the KHP is 0.7840 g. Before the titration the buret reading was 0.8400 mL and afterwards it was 39.20 mL. A 85.12 mL sample of a solution of sulfuric acid, H2SO4, is neutralized by 59.82 mL of the NaOH solution from the problem above. Calculate the molarity of the sulfuric acid solution.

What is the percent acetic acid in a 50.0 mL sample, which required 45.0 mL of a 0.1466 M NAOH to reach the equivalence point? (The sample solution has a density of 1.090 g/mL.) CH;CO,H(aq) - N2OH(aq) – NaCH;CO,(aq) - H,0(1)

Macmillar For the chemical reaction HCN(aq) + KOH(aq) → H,O(l) + KCN(aq) write the net ionic equation, including the phases. net ionic equation:

Sodium hydrogen carbonate (NaHCO3), also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid (HCI), which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO, neutralizes excess HCI through this reaction: HCl(aq) + NaHCO3(aq) NaCl(aq) + H₂O(1) + CO₂(g) The CO₂ gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a man suffering from indigestion can be considered to be 200 ml of a 0.050 M HCI solution. What mass of NaHCO, would he need to ingest to neutralize this much HCI? Be sure your answer has the correct number of significant digits. X

6 a b U d [Tutorial: Titration stoichiometry] This question will walk you through the steps of calculating the volume of titrant required to reach the endpoint based on the volume and concentration of analyte. Consider the standardization of NaOH by titration with C,H,O, according to the following chemical reaction: 3 NaOH(aq) + C,H,O,(aq) = Na,C,H,O,(aq) + 3 H₂O(l) Step 1: Evaluate the question. How many moles of aqueous sodium hydroxide (NaOH) will react to completely neutralize one mole of aqueous citric acid (C,H,O,)? Which equation will be most helpful for solving this problem? Calculate the volume in mL of a 0.200 M NaOH solution needed to neutralize 345 mL of 0.033 MC,H,O, standard solution. Based on the fact that NaOH is a strong base and C,H,O, is a weak acid, how would you describe the pH of the solution at the endpoint, where moles of base = 3 times the moles of acid?

How to write a balance equation from H2C3H5O3 (aq) + KOH (aq)

Given the following information: hydrocyanic acid Ka = 4.0E-10 HCN HF hydrofluoric acid Ka = 7.2E-4 (1) Write the net ionic equation for the reaction that occurs when equal volumes of 0.236 M aqueous hydrocyanic acid and sodium fluoride are mixed. It is not necessary to include states such as (aq) or (s). A₂ A² A₂ A² A₂ A² A₂ A² (2) At equilibrium the ✓will be favored. (3) The pH of the resulting solution will be seven.