I need help on the problems below.. Please feel free to correct my work, thank you **Balancing Chemical Equations: Educational Exercise**1) **Equation**: \[ \text{Ni(s)} + \text{__ H}_2\text{SO}_4\text{(aq)} \rightarrow \text{__ NiSO}_4\text{(aq)} + \text{__ H}_2\text{(g)} \]2) **Instruction**: Balance and write net ionic chemical equations for each of the following reactions.**Reaction 1**: \[ \text{__ H}_3\text{PO}_4\text{(aq)} + \text{3 LiOH(aq)} \rightarrow \text{__ Li}_3\text{PO}_4\text{(aq)} + \text{3 H}_2\text{O(l)} \]**Note**: The coefficients have been indicated above as "3 OH\text{(aq)} + 3 Li\text{(aq)} + H_3PO_4\text{(aq)} \rightarrow 3 Li_3PO_4\text{(aq)} + 3 H}_2\text{O(l)}". This seems to be an error as the products do not balance the equation properly. Please ensure proper balancing of both sides.**Annotation**: "3 OH" and "3 Li" indicate the individual ions separated in solution, implying an understanding of ionic equations and how compounds dissociate in water.**Reaction 2**: \[ \text{Sr(s)} + \text{__ H}_2\text{O(l)} \rightarrow \text{__ Sr(OH)}_2\text{(aq)} + \text{__ H}_2\text{(g)} \]**General Tips for Balancing**:- Write down the number of each type of atom present in the unbalanced equation.- Use coefficients to balance the metals, non-metals, and lastly, hydrogen and oxygen.- Ensure the total charge is the same on both sides for ionic equations. **Visual Features**:- No graphs or diagrams present in the image.- Handwritten notes providing clues for correct balancing.- Ensure accuracy when translating handwritten notes to digital formats.This exercise helps in understanding the principles of chemical reactions, stoichiometry, and conservation of mass and charge.

To balance a reaction, we need to count each atoms and make them equal in both reactant side and product side. A net ionic equation is the chemical equation that only shows the compounds or ions which take part in the reaction. 1. H3 PO 4 + Li OH --> Li 3 PO 4 + H2 O : To balance the reaction, we need to count each atoms. Reactant side product side H 4 2 P 1 1 O 5 5 Li 1 3 To make both sides equal, we need to multiply the equation with certain integers. Thus, the balanced equation is : H3 PO 4 + 3 LiOH --> Li3 PO 4 + 3 H2 O In the reaction, Lithium phosphate is water soluble, so Li+ (aq), PO 43- (aq) are spectator ions. Cancelling them in both sides, we can write the net ionic equation. The net ionic equation is : 3 OH - (aq) + 3 H+ (aq) --> 3 H2 O (l) 2. Sr (s) + H2 O (l) --> Sr( OH) 2 (aq) + H2 (g) : This is a redox reaction, where metal is oxidised, and water is reduced to hydrogen gas. The balanced equation is : Sr + 2 H2 O --> Sr(OH) 2 + H2 Now if we write the total ionic equation, then : Sr (s) + 2 H+ (aq) + 2 OH- (aq) --> Sr 2+ (aq) + 2 OH - (aq) + H2 (g) Cancelling the spectator ion , the net ionic equation can be written as below : Sr (s) + 2 H+ (aq) --> Sr 2+(aq) + H2 (g)